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All Textbook Solutions for Chemistry by OpenStax (2015-05-04)

Suggest an explanation for the observations that ethanol, C2H5OH, is completely miscible with water and that ethanethiol, C2H5SH, is soluble only to the extent of 1.5 g per 100 mL of water.Calculate the percent by mass of KBr in a saturated solution of KBr in water at 10 °C. See Figure 11.17 for useful data, and report the computed percentage to one significant digit.Which of the following gases is expected to be most soluble in water? Explain your reasoning. (a) CH4 (b) CCI4 (c) CHCI3 At 0 C and 1.00 atm, as much as 0.70 g of O2 can dissolve in 1 L of water. At 0 C and 4.00 atm, how many grams of O2 dissolve in 1 L of water?Refer to Figure 11.11. (a) How did the concentration of dissolved CO2 in the beverage change when the bottle was opened? (b) What caused this change? (c) Is the beverage unsaturated, saturated, or supersaturated with CO2?The Henry's law constant for CO2 is 3.4102 M/atm at 25 C. What pressure of carbon dioxide is needed to maintain a CO2 concentration of 0.10 M in a can of lemon-lime soda?The Henry's law constant for O2 is 1.3103M /atm at 25 C. What mass of oxygen would be dissolved in a 40-L aquarium at 25 C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of O2 is 0.21 atm?How many liters of HCI gas, measured at 30.0 C and 745 torr, are required to prepare 1.25 L of a 3.20-M solution of hydrochloric acid?Which is are part of the macroscopic domain of solutions and which is are part of the microscopic domain: boiling point elevation, Henry's law, hydrogen bond, ion-dipole attraction, molarity, nonelectrolyte, nonstoichiometric compound, osmosis, solvated ion?What is the microscopic explanation for the macroscopic behaviour illustrated in Figure 11.15?Sketch a qualitative graph of the pressure versus time for water vapor above a sample of pure water and a sugar solution, as the liquids evaporate to half their original volume.A solution of potassium nitrate, an electrolyte, and a solution of glycerin (C3H5(OH)3), a nonelectrolyte, both boil at 100.3 C. What other physical properties of the two solutions are identical?What are the mole fractions of H3PO4 and water in a solution of 14.5 g of H3PO4 in 125 g of water? (a) Outline the steps necessary to answer the question. (b) Answer the question.What are the mole fractions of HNO3 and water in a concentrated solution of nitric acid (68.0% HNO3 by mass)? (a) Outline the steps necessary to answer the question. (b) Answer the question.Calculate the mole fraction of each solute and solvent: (a) 583 g of H2SO4 in 1.50 kg of water—the acid solution used in an automobile battery (b) 0.86 g of NaCl in 1.00102 g of water—a solution of sodium chloride for intravenous injection (c) 46.85 g of codeine, C18H21NO3, in 125.5 g of ethanol, C2H5OH (d) 25 g of I2 in 125 g of ethanol, C2H5OH Calculate the mole fraction of each solute and solvent: (a) 0.710 kg of sodium carbonate (washing soda), Na2CO3, in 10.0 kg of water—a saturated solution at 0 C (b) 125 g of NH4NO3 in 275 g of water—a mixture used to make an instant ice pack (c) 25 g of CI2 in 125 g of dichloromethane, CH2CI2 (d) 0.372 g of tetrahydropyridine, C5H9N, in 125 g of chloroform, CHCI3 Calculate the mole fractions of methanol, CH3OH; ethanol, C2H5OH; and water in a solution that is 40% methanol, 40% ethanol, and 20% water by mass. (Assume the data are good to two significant figures.)What is the difference between a 1 M solution and a 1 m solution?What is the molality of phosphoric acid, H3PO4, in a solution of 14.5 of H3PO4 in 125 g of water? (a) Outline the steps necessa1Y to answer the question. (b) Answer the question.What is the molality of nitric acid in a concentrated solution of nitric acid (68.0% HNO3 by mass)? (a) Outline the steps necessary to answer the question. (b) Answer the question.Calculate the molality of each of the following solutions: (a) 583 g of H2SO4 in 1.50 kg of water—the acid solution used in an automobile battery (b) 0.86 g of NaCI in 1.00102 g of water—a solution of sodium chloride for intravenous injection (c) 46.85 g of codeine, C18H21NO3, in 125.5 g of ethanol, C2H5OH (d) 25 g of I2 in 125 g of ethanol, C2H5OH Calculate the molality of each of the following solutions: (a) 0.710 kg of sodium carbonate (washing soda), Na2CO3, in 10.0 kg of water—a saturated solution at 0C (b) 125 g of NH4NO3 in 275 g of water—a mixture used to make an instant ice pack (c) 25 g of CI2 in 125 g of dichloromethane, CH2CI2 (d) 0.372 g of tetrahydropyridine, C5H9N, in 125 g of chloroform, CHCI3 The concentration of glucose, C6H12O6, in normal spinal fluid is 75mg100mg. What is the molality of the solution?A 13.0% solution of K2CO3 by mass has a density of 1.09 g/cm3. Calculate the molality of the solution.Why does 1 mol of sodium chloride depress the freezing point of 1 kg of water almost twice as much as 1 mol of glycerin?What is the boiling point of a solution of 115.0 g of sucrose, C12H22O11, in 350.0 g of water? (a) Outline the steps necessary to answer the question (b) Answer the question What is the boiling point of a solution of 9.04 g of I2 in 75.5 g of benzene, assuming the I2 is nonvolatile? (a) Outline the steps necessary to answer the question. (b) Answer the question.What is the freezing temperature of a solution of 115.0 g of sucrose, C12H22O11, in 350.0 g of water, which freezes at 0.0 C when pure? (a) Outline the steps necessary to answer the question. (b) Answer the question.What is the freezing point of a solution of 9.04 g of I2 in 75.5 g of benzene? (a) Outline the steps necessary to answer the following question. (b) Answer the question.What is the osmotic pressure of an aqueous solution of 1.64 g Ca(NO3)2 of in water at 25 C? The volume of the solution is 275 mL. (a) Outline the steps necessa1Y to answer the question. (b) Answer the question.What is osmotic pressure of a solution of bovine insulin (molar mass, 5700 g mol-1) at 18 C if 100.0 mL of the solution contains 0.103 g of the insulin? (a) Outline the steps necessary to answer the question. (b) Answer the question.What is the molar mass of a solution of 5.00 g of a compound in 25.00 g of carbon tetrachloride (bp 76.8 C; Kb=5.02 C/m) that boils at 81.5 C at 1 atm? (a) Outline the steps necessa1Y to answer the question. (b) Solve the problem.A sample of an organic compound (a nonelectrolyte) weighing 1.35 g lowered the freezing point of 10.0 of benzene by 3.66 C. Calculate the molar mass of the compound.A 1.0 m solution of HCI in benzene has a freezing point of 0.4 C. Is HCI an electrolyte in benzene? Explain.A solution contains 5.00 g of urea, CO(NH2)2, a nonvolatile compound, dissolved in 0.100 kg of water. If the vapor pressure of pure water at 25 C is 23.7 torr, what is the vapor pressure of the solution?A 12.0-g sample of a nonelectrolyte is dissolved in 80.0 g of water. The solution freezes at -1.94 C. Calculate the molar mass of the substance.Arrange the following solutions in order by their decreasing freezing points: 0.1 m Na3PO4, 0.1 m C2H5OH, 0.01 m CO2, 0.151 m NaCI, and 0.21 m cacI2.Calculate the boiling point elevation of 0.100 kg of water containing 0.010 mol of NaCl, 0.020 mol of Na2SO4, and 0.030 mol of MgCI2, assuming complete dissociation of these electrolytes.How could you prepare a 3.08 m aqueous solution of glycerin, C3H8O3? What is the freezing point of this solution?A sample of sulfur weighing 0.210 g was dissolved in 17.8 g of carbon disulfide, CS2 ( Kb=2.43 C/m). If the boiling point elevation was 0.107 C, what is the formula of a sulfur molecule in carbon disulfide?In a significant experiment performed many years ago, 5.6977 g of cadmium iodide in 44.69 g of water raised the boiling point 0.181 C. What does this suggest about the nature of a solution of CdI2?Lysozyme is an enzyme that cleaves cell walls. A 0.100-L sample of a solution of lysozyme that contains 0.0750 g of the enzyme exhibits an osmotic pressure of 1.32103 atm at 25 C. What is the molar mass of lysozyme?The osmotic pressure of a solution containing 7.0 g of insulin per liter is 23 torr at 25 C. What is the molar mass of insulin?The osmotic pressure of human blood is 7.6 atm at 37 C. What mass of glucose, C6H12O6, is required to make 1.00 L of aqueous solution for intravenous feeding if the solution must have the same osmotic pressure as blood at body temperature, 37 C?What is the freezing point of a solution of dibromobenzene, C6H4Br2, in 0.250 kg of benzene, if the solution boils at 83.5 C?What is the boiling point of a solution of NaCI in water if the solution freezes at -0.93 C?The sugar fructose contains 40.0% C, 6.7% H, and 53.3% O by mass. A solution of 11.7 g of fructose in 325 g of ethanol has a boiling point of 78.59 C. The boiling point of ethanol is 78.35 C, and Kb for ethanol is 1.20 C/m . What is the molecular formula of fructose?The vapor pressure of methanol, CH3OH, is 94 torr at 20 C. The vapor pressure of ethanol, C2H5OH, is 44 torr at the same temperature. (a) Calculate the mole fraction of methanol and of ethanol in a solution of 50.0 g of methanol and 50.0 g of ethanol. (b) Ethanol and methanol form a solution that behaves like an ideal solution. Calculate the vapor pressure of methanol and of ethanol above the solution at 20 C.The triple point of air-free water is defined as 273.16 K. Why is it important that the water be free of air?Meat can be classified as fresh (not frozen) even though it is stored at -1 C. Why wouldn't meat freeze at this temperature?An organic compound has a composition of 93.46% C and 6.54% H by mass. A solution of 0.090 g of this compound in 1.10 g of camphor melts at 158.4 C. The melting point of pure camphor is 178.4 C. Kf for camphor is 37.7 C/m . What is the molecular formula of the solute? Show your calculations.A sample of HgCI2 weighing 9.41 g is dissolved in 32.75 g of ethanol, C2H5OH ( Kb=1.20 C/m). The boiling point elevation of the solution is 1.27 C. Is HgCI2 an electrolyte in ethanol? Show your calculations.A salt is known to be an alkali metal fluoride. A quick approximate determination of freezing point indicates that 4 g of the salt dissolved in 100 g of water produces a solution that freezes at about -1.4 C. What is the formula of the salt? Show your calculations.Identify the dispersed phase and the dispersion medium in each of the following colloidal systems: starch dispersion, smoke, fog, pearl, whipped cream, floating soap, jelly, milk, and ruby.Distinguish between dispersion methods and condensation methods for preparing colloidal systems.How do colloids differ from solutions with regard to dispersed particle size and homogeneity?Explain the cleansing action of soap.How can it be demonstrated that colloidal particles are electrically charged?What is the difference between average rate, initial rate, and instantaneous rate?Ozone decomposes to oxygen according to the equation 2O3(g)3O2(g). Write the equation that relates the rate expressions for this reaction in terms of the disappearance of O3 and the formation of oxygen.In the nuclear industry, chlorine trifluoride is used to prepare uranium hexafluoride, a volatile compound of uranium used in the separation of uranium isotopes. Chlorine trifluoride is prepared by the reaction CI2(g)+3F2(g)2CIF3(g). Write the equation that relates the rate expressions for this reaction in terms of the disappearance of Cl2 and F2 and the formation of CIF3.A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).A study of the rate of the reaction represented as 2AB gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 35.0 [A](M) 1.00 0.775 0.625 0.465 0.350 0.205 0.230 (a) Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0 s and 20.0 s. (b) Estimate the instantaneous rate of disappearance of A at 15.0 s from a graph of time versus [A]. What are theunits of this rate? (c) Use the rates found in parts (a) and (b) to determine the average rate of formation of B between 0.00 s and 10.0 s, and the instantaneous rate of formation of B at 15.0 s.Consider the following reaction in aqueous solution: 5Br(aq)+BrO3(aq)+6H+(aq)3Br2(aq)+3H2O(l) If the rate of disappearance of Br(aq) at a particular moment during the reaction is 3.5104Ms1, what is the rate of appearance of 3Br2(aq) at that moment?Describe the effect of each of the following on the rate of the reaction of magnesium metal with a solution of hydrochloric acid: the molarity of the hydrochloric acid, the temperature of the solution, and the size of the pieces of magnesium.Explain why an egg cooks move slowly in boiling water in Denver than in New York City. (Hint: Consider the effect 0f temperature on reaction rate and the effect of pressure on boiling point.)Go to the PhET Reactions and change to Angled shot to see the difference. (a) What happens when the angle of the collision is changed? (b) Explain how this is relevant to rate of reaction.In the PhET Reactions tab to observe how multiple atoms and molecules interact under varying conditions. Select a molecule to pump into the chamber. Set the initial temperature and select the current amounts of each reactant. Select Show bonds under Options. How is the rate of the reaction affected by concentration and temperature?In the PhET Reactions under Options. (a) Leave the Initial Temperature at the default setting. Observe the reaction. Is the rate of reaction fast or slow? (b) Click Pause" and then Reset All, and then enter 15 molecules of A and 10 molecules of BC once again. Select Show Bonds" under Options. This time, increase the initial temperature until, on the graph, the total average energy line is completely above the potential energy curve. Describe what happens to the reaction.How do the rate of a reaction and its rate constant differ?Doubling the concentration of a reactant increases the rate of a reaction four times. With this knowledge, answer the following questions: (a) What is the order of the reaction with respect to that reactant? (b) Tripling the concentration of a different reactant increases the rate of a reaction three times. What is the order of the reaction with respect to that reactant?Tripling the concentration of a reactant increases the rate of a reaction nine times. With this knowledge, answer the following questions: (a) What is the order of the reaction with respect to that reactant? (b) Increasing the concentration of a reactant by a factor of four increases the rate of a reaction four times. What is the order of the reaction with respect to that reactant?How much and in what direction will each of the following affect the rate of the reaction: CO(g)+NO2CO2(g)+NO(g) if the rate law for the reaction is rate =k[NO2]2? (a) Decreasing the pressure of NO2 from 0.50 atm to 0.250 atm. (b) Increasing the concentration of CO from 0.01 M to 0.03 M.How will each of the following affect the rate of the reaction: CO(g)+NO2CO2(g)+NO(g) } if the rate law for the reaction] is rate =k[NO2][CO]? (a) Increasing the pressure of NO2 from 0.1 atm to 0.3 atm (b) Increasing the concentration of CO from 0.02 M to 0.06 M.Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?Radioactive phosphorus is used in the study of biochemical reaction mechanisms because phosphorus atoms are components of many biochemical molecules. The location of the phosphorus (and the location of the molecule it is bound in) can be detected from the electrons (beta particles) it produces: P1532S1632+e Rate =4.85102day1[32P] What is the instantaneous rate of production of electrons in a sample with a phosphorus concentration of 0.0033 M?The rate constant for the radioactive decay of 14C is 1.21104 year-1. The products of the decay are nitrogen atoms and electrons (beta particles): C614N714+e rate =k[C614] What is the instantaneous rate of production of N atoms in a sample with a carbon-14 content of 6.5109M?The decomposition of acetaldehyde is a second order reaction with a rate constant of 4.71108 L/mol/s. What is the instantaneous rate of decomposition of acetaldehyde in a solution with a concentration of 5.55104M?Alcohol is removed from the bloodstream by a series of metabolic reactions. The first reaction produces acetaldehyde; then other products are formed. The following data have been determined for the rate at which alcohol is removed from the blood of an average male, although individual rates can vary by 2530%. Women metabolize alcohol a little more slowly than men: [C2H5OH](M) 4.4102 3.3102 2.2102 Rate(moI/L/h) 2.0102 2.0102 2.0102 Determine the rate equation, the rate constant, and the overall order for this reaction.Under certain conditions the decomposition of ammonia on a metal surface gives the following data: [NH3] (M) 1.0103 2.0103 3.0103 Rate (moI/L/h1) 1.5106 1.5106 1.5106 Determine the rate equation, the rate constant, and the overall order for this reaction.Nitrosyl chloride, NOCI, decomposes to NO and CI2. 2NOCI(g)2NO(g)+CI2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.20 0.30 Rate (mol/L/h) 8.01010 3.2109 7.2109 From the following data, determine the rate equation, the rate constant, and the order with respect to A for the reaction A2C. [A](M) 1.33102 2.66102 3.99102 Rate (mol/L/h) 3.80107 1.52106 3.42106 Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation: H2(g)+2NO(g)N2O(g)+H2O(g) Determine the rate equation, the rate constant, and the orders with respect to each reactant from the following data: [NO] (M) 0.30 0.60 0.60 [H2] (M) 0.35 0.35 0.70 Rate (mol/L/s) 2.835103 1.134102 2.268102 For the reaction AB+C, the following data were obtained at 30 C: [A] (M) 0.230 0.356 0.557 Rate (moI/L/s) 4.17104 9.99104 2.44103 (a) What is the order of the reaction with respect to [A], and what is the rate equation? (b) What is the rate constant?For the reaction QW+X, the following data were obtained at 30 C: [Q]initial (M) 0.170 0.212 0.357 Rate(mol/L/s) 6.68103 1.04102 2.94102 (a) What is the order of the reaction with respect to [Q], and what is the rate equation? (b) What is the rate constant?The rate constant for the ?rst-order decomposition at 45 C of dinitrogen pentoxide, N2O5, dissolved in chloroform, CHCI3, is 6.2104 min-1. 2N2O54NO2+O2 What is the rate of the reaction when [N2O5] = 0.40 M?The annual production of HNO3 in 2013 was 60 million metric tons Most of that was prepared by the following sequence of reactions, each run in a separate reaction vessel. (a) 4NH3(g)+5O2(g)4NO(g)+6H2O(g) (b) 2NO(g)+O2(g)2NO2(g) (C) 3NO2(g)+H2O(l)2HNO3(aq)+NO(g) The first reaction is run by burning ammonia in air over a platinum catalyst. This reaction is fast. The reaction in equation (c) is also fast. The second reaction limits the rate at which nitric acid can be prepared from ammonia. If equation (b) is second order in NO and first order in O2, what is the rate of formation of NO2 when the oxygen concentration is 0.50 M and the nitric oxide concentration is 0.75 M? The rate constant for the reaction is 5.8106 L2/mol2/s.The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI] 0.050 0.050 0.010 Rate(mol/L/s) 3.05104 6.20104 1.83104 Determine the rate equation and the rate constant for this reaction.Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.Use the data provided to graphically determine the order and rate constant of the following reaction: SO2CI2SO2+CI2 Time(s) 0 5.00103 1.00104 1.50104 [SO2CI2] (M) 0.100 0.0896 0.0802 0.0719 Time(s) 2.50104 3.00104 4.00104 [SO2CI2] (M) 0.0577 0.0517 0.0415 Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103 Pure ozone decomposes slowly to oxygen, 2O33O2(g). Use the data provided in a graphical method and determine the order and rate constant of the reaction. Time (h) 0 2.0103 7.6103 1.00104 [O3](M) 1.00105 4.98106 2.07106 1.66106 Time (h) 1.23104 1.43104 1.70104 [O3](M) 1.39106 1.22106 1.05106 From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2XY+Z Time (s) 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 [X](M) 0.0990 0.0497 0.0332 0.0249 0.0200 0.0166 0.0143 0.0125 What is the half-life for the first-order decay of phosphorus-32? (P1532S1632+e) The rate constant for the decay is 4.85102 day-1.What is the half-life for the first-order decay of carbon-14? (C614N714+e) The rate constant for the decay is 1.21102 year-1.What is the half-life for the decomposition of NBCI when the concentration of NOCI is 0.15 M? The rate constant for this second-order reaction is 8.0108 L/mol/s.What is the half-life for the decomposition of O3 when the concentration of O3 is 2.35106M? The rate constant for this second-order reaction is 50.4 L/mol/h.The reaction of compound A to give compounds C and D was found to be second-order in A . The rate constant for the reaction was determined to be 2.42 L/mol/s. If the initial concentration is 0.500 mol/L, what is the value of t1/2?The half-life of a reaction of compound A to give compounds D and E is 8.50 min when the initial concentration of A is 0.150 mol/L. How long will it take for the concentration to drop to 0.0300 mol/L if the reaction is (a) first order with respect to A or (b) second order with respect to A?Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010 Both technetium-99 and thallium-201 are used to image heart muscle in patients with suspected heart problems. The half-lives are 6 h and 73 h, respectively. What percent of the radioactivity would remain for each of the isotopes after 2 days (48 h)?There are two molecules with the formula C3H6 Propane, CH3CH = CH2, is the monomer of the polymer polypropylene, which is used for indoor-outdoor carpets. Cyclopropane is used as an anesthetic: When heated to 499 C, cyclopropane rearranges (isomerizes) and forms propane with a rate constant of 5.95104s1. What is the half-life of this reaction? What fraction of the cyclopropane remains after 0.75 h at 499 C?Fluorine-18 is a radioactive isotope that decays by positron emission to form oxygen-18 with a half-life of 109.7 min. (A positron is a particle with the mass of an electron and a single unit of positive charge; the equation is F918O188+e+10 Physicians use 18F to study the brain by injecting a quantity of ?uoro-substituted glucose into the blood of a patient. The glucose accumulates in the regions where the brain is active and needs nourishment. (a) What is the rate constant for [lie decomposition of ?uorine-18? (b) If a sample of glucose containing radioactive fluorine-18 is injected into the blood, what percent of the radioactivity will remain after 5.59 h? (c) How long does it take for 99.99% of the 18F to decay?Suppose that the half-life of steroids taken by an athlete is 42 days. Assuming that the steroids biodegrade by a first-order process 5, how long would it take for 164 of the initial dose to remain in the athlete’s body?Recently, the skeleton of King Richard III was found under a parking lot in England. If tissue samples from the skeleton) contain about 93.79% of the carbon-14 expected in living tissue, what year did King Richard III die? The half-life fur carbon-14 is 5730 years.Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4 For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.Chemical reactions occur when reactants collide. What are two factors that may prevent a collision from producing a chemical reaction?When every collision between reactants leads to a reaction, what determines the rate at which the reaction occurs?What is the activation energy of a reaction, and how is this energy related to the activated complex of the reaction?Account for the relationship between the rate of a reaction and its activation energy.Describe how graphical methods can be used to determine the activation energy of a reaction from a series of data that includes the rate of reaction at varying temperatures.How does an increase in temperature affect rate of reaction? Explain this effect in terms of the collision theory of the reaction rate.The rate of a certain reaction doubles for every 10 C rise in temperature. (a) How much faster does the reaction proceed at 45 C than at 25 C? (b) How much faster does the reaction proceed at 95 C than at 25 C?In an experiment, a sample of NaClO3 was 90% decomposed in 48 min. Approximately how long would this decomposition have taken if the sample had been heated 20 C higher? (Hint: Assume the rate doubles for each 10 C rise in temperature.)The rate constant at 325 C for the decomposition reaction C4H82C2H4 is 6.1108s1, and the activation energy is 261 kJ per mole of C4H8. Determine the frequency factor for the reaction.The rate constant for the decomposition of acetaldehyde, CH3CHO, t0 methane, CH4, and carbon monoxide, CO, in the gas phase is 1.1102 L/mol/s at 703 K and 4.95 L/moI/s at 865 K. Determine the activation energy for this decomposition.An elevated level of the enzyme alkaline phosphatase (ALP) in human serum is an indication of possible liver or bone disorder. The level of serum ALP is so low that it is very difficult to measure directly. However. ALP catalyzes a number of reactions, and its relative concentration can be determined by measuring the rate of one of these reactions under controlled conditions. One such reaction is the conversion of p-nitrophenyI phosphate (PNPP) to p-nitrophenoxide ion (PNP) and phosphate ion. Control of temperature during the test is very important; the rate of the reaction increases 1.47 times if the temperature changes from 30 C to 37 C. What is the activation energy for the ALP-catalyzed conversion of PNPP to PNP and phosphate?In terms of collision theory, to which of the following is the rate of a chemical reaction proportional? (a) the change in free energy per second (b) the change in temperature per second (c) the number of collisions per second (d) the number of product molecules Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?The element Co exists in two oxidation states, Co(II) and Co(III), and the ions form many complexes. The rate at which one of the complexes of Co(III) was reduced by Fe(II) in water was measured. Determine the activation energy of the reaction from the following data: T(K) k (s-1) 293 0.054 298 0.100 The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?Use the PhET Reactions Single collision" tab of the simulation applet, enable the Energy view by clicking the + icon. Select the first A+BCAB+C reaction] (A is yellow, B is purple, and C is navy blue). Using the straight shot default option, try launching the A atom with varying amounts of energy. What changes when the Total Energy line at launch is below the transition state of the Potential Energy line? Why? What happens when it is above the transition state? Why?Use the PhET Reactions Single collision tab of the simulation applet, enable the Energy view" by clicking the + icon. Select the first A+BCAB+C reaction (A is yellow, B is purple. and C is navy blue). Using the angled shut option, try launching the A atom with varying angles, but with more Total energy than the transition state. What happens when the A atom hits the BC molecule from different directions? Why?Why awe elementary reactions involving three or more reactants very uncommon?In general, can we predict the effect of doubling the concentration of A on the rate of the overall reaction A+BC? Can we predict the effect if the reaction is known to be an elementary reaction?Define these terms: (a) unimolecular reaction (b) bimolecular reaction (c) elementary reaction (d) overall reaction What is the rate equation for the elementary termolecular reaction A+2B products? For 3A products?Given the following reactions and the corresponding rate laws, in which of the reactions might the elementary reaction and the overall reaction be the same? (a) Cl2+COCI2COrate=k[ CI2]3/2[CO] (b) PCI3+CI2PCI5rate=k[PCI3][CI2] (c) 2NO+H2N2+H2Orate=k[NO][H2] (d) 2NO+O22NO2rate=k[NO]2[O2] (e) NO+O3NO2+O2rate=k[NO][O3]Write the rate equation for each of the following elementary reactions: (a) O3sunlightO2+O (b) O3+CIO2+CIO (c) CIO+OCI+O2 (d) O3+NONO2+O2 (e) NO2+ONO+O2 Nitrogen (Il) oxide, NO, reacts with hydrogen, H2, according to the following equation: 2NO+2H2N2+2H2O What would the rate law be if the mechanism for this reaction were: 2NO+H2N2+H2O2 (slow) H2O2+H22H2O (fast)Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2NO(g)+2H2(g)N2(g)+2H2O(g) Initial concentrations and rates of reaction are given here. Experiment Initial Concentration [NO] (mol/L) Initial Concentration, [H2] (mol/L) Initial Rate of Formation of N2 (mol/L min) 1 0.0060 0.0010 1.8104 2 0.0060 0.0020 3.6104 3 0.0010 0.0060 0.30104 4 0.0020 0.0060 1.2104 Consider the following questions: (a) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning. (b) Write the overall rate law for the reaction. (c) Calculate the value of the rate constant, k, for the reaction. Include units. (d) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H2 had been consumed. (e) The following sequence of elementary steps is a proposed mechanism for the reaction. Step 1: NO+NON2O2 Step 2: N2O2+H2H2O+N2O Step 3: N2O+H2N2+H2O Based on the data presented, which of these is the rate determining step? Show that the mechanism is consistent with the observed rate law for the reaction and the overall stoichiometry of the reaction.The reaction of CO with CI2 gives phosgene (COCI2), a nerve gas that was used in World War I. Use the mechanism shown here to complete the following exercises: CI2(g)2CI(g) (fast, k1 represents the forward rate constant, k-1 the reverse rate constant) CO(g)+CI(g)COCI(g) (slow, k2 the rate constant) COCI(g)+CI(g)COCI2(g) (fast, k3 the rate constant) (a) Write the overall reaction. (b) Identify all intermediates. (c) Write the rate law for each elementary reaction. (d) Write the overall rate law expression.. Account for the increase in reaction rate brought about by a catalyst.Compare the functions of homogeneous and heterogeneous catalysts.Consider this scenario and answer the following questions: Chlorine atoms resulting from decomposition of chloro?uoromethanes, such as CCI2F2, catalyze the decomposition of ozone in the atmosphere. One simplified mechanism for the decomposition is: O3sunlightO2+O O3+CIO2+CIO CIO+OCI+O2 (a) Explain why chlorine atoms are catalysts in the gas-phase transformation: 2O33O2 (b) Nitric oxide is also involved in the decomposition of ozone by the mechanism: O3sunlightO2+O O3+NONO2+O2 NO2+ONO+O2 Is NO a catalyst for the decomposition? Explain your answer.For each of the following pairs of reaction diagrams, identify which of the pair is catalyzed:For each of the following pairs of reaction diagrams, identify which of the pairs is catalyzed:For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:Based on the diagrams in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?Based on the diagram in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?What does it mean to describe a reaction as reversible?When writing an equation, how is a reversible reaction distinguished from a nonreversible reaction?If a reaction is reversible, when can it be said to have reached equilibrium?Is a system at equilibrium if the rate constants of the forward and reverse reactions are equal?If the concentrations of products and reactants are equal, is the system at equilibrium?Explain why there may be an infinite number of values for the reaction quotient of a reaction at a given temperature but theme can he only one value for the equilibrium constant at that temperature.Explain why an equilibrium between Br2(l) and Br2(g) would not be established if the container were not a closed vessel shown in Figure 13.5.If you observe the following reaction at equilibrium, is it possible to tell whether the reaction stated with pure NO2 or with pure N2O4? 2NO2(g)N2O4(g)Among the solubility rules previously discussed is the statement: All chlorides are soluble except Hg2Cl2, AgCI, PbCl2, and CuCl. (a) Write the expression for the equilibrium constant for the reaction represented by the equation AgCI(s)Ag+CI(aq). Is Kc1,1, or 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation Pb2+(aq)+2CI(aq)PbCI2(s). Is Kc1,1, or 1? Explain your answer.Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, and arsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equation CaCO3(s)Ca2+(aq)+CO32(aq). Is Kc1,1, or 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation 3Ba2+(aq)+2PO43(aq)Ba3( PO4)2(s). Is Kc1,1, or 1? Explain your answer.Benzene is one of the compounds used as octane enhancers in unleaded gasoline. It is manufactured by the catalytic conversion of acetylene to benzene: 3C2H2(g)C6H6(g). Which value of Kc would make this reaction most useful commercially? Kc0.01,Kc1, or Kc10. Explain your answer.Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Kc1,1, or 1 for a titration reaction?For a precipitation reaction to be useful in a gravimetric analysis, the product of the reaction must be insoluble. Is Kc1,1 or 1 for a useful precipitation reaction?Write the mathematical expression for the reaction quotient, QC, for each of the following reactions: (a) CH4(g)+CI2CH3CI(g)+HCI(g) (b) N2(g)+O2(g)2NO(g) (c) 2SO2(g)+O2(g)2SO3(g) (d) BaSO3(s)BaO(s)+SO2(g) (e) P4(g)+5O2(g)P4O10(s) (f) Br2(g)2Br(g) (g) CH4(g)+2O2(g)CO2(g)+2H2O(l) (h) CuSO45H2O(s)CuSO4(s)+5H2O(g)Write the mathematical expression for the reaction quotient, QC, for each of the following reactions (a) N2(g)+3H2(g)2NH3(g) (b) 4NH3(g)+5O2(g)4NO(g)+6H2O(g) (C) N2O2(g)2NO2(g) (d) CO2(g)+H2CO(g)+H2O(g) (e) NH4CI(s)NH3(g)+HCI(g) (f) 2Pb( NO3)2(s)2PbO(s)+4NO2(g)+O2(g) (g) 2H2(g)+O2(g)2H2O(g) (h) S8(g)8S(g)The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction] in which each system will proceed to leach equilibrium. (a) 2NH3(g)N2(g)+3H2(g) Kc=17;[NH3]=0.20M,[N2]=1.00M,[H2]=1.00M (b) 2NH3(g)N2(g)+3H2(g) Kp=6.8104 initial pressures NH3=3.0atm,N2=2.0atm,H2=1.0atm (c) 2SO3(g)2SO2(g)+O2(g) Kc=0.230;[SO3]=0.00M,[SO2]=1.00M,[O2]=1.00M (d) 2SO3(g)2SO2(g)+O2(g) Kp=16.5 initial pressures SO3=1.00atm,SO2=1.00atm,O2=1.00atm (e) 2NO(g)+CI2(g)2NOCI(g) Kc=4.6104;[NO]=1.00M,[CI2]=1.00M,[NOCI]=0M (f) N2(g)+O2(g)2NO(g) Kp=0.050 initial pressures NO=1.00atm,N2=O2=5atm The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (a) 2NH3(g)N2(g)+3H2(g) Kc=17;[NH3]=0.50M,[N2]=0.15M,[H2]=0.12M (b) 2NH3(g)N2(g)+3H2(g) Kp=6.8104 initial pressures NH3=2.00atm,N2=10.00atm,H2=10.00atm (c) 2SO3(g)2SO2(g)+O2(g) Kc=0.230;[SO3]=2.00M,[SO2]=2.00M,[O2]=2.00M (d) 2SO3(g)2SO2(g)+O2(g) Kp=16.5 initial pressures SO2=1.00atm,O2=1.130atm,SO3=0atm (e) 2NO(g)+CI2(g)2NOCI(g) Kp=2.5103 ; initial pressures; NO=1.00atm,CI2=1.00atm,NOCI=0atm (f) N2(g)+O2(g)2NO(g) Kc=0.050 ; [N2]=1.00M,[O2]=0.200M,[NO]=1.00M The following reaction has KP=4.50105 at 720 K. N2(g)+3H2(g)2NH3 If a reaction vessel is filled with each gas to the partial pressures listed, in which direction will it shift to reach equilibrium? P(NH3)=93atm,P(N2)=48atm, and P(H2)=52 Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to each equilibrium? SO2CI2(g)SO2(g)+CI2(g) [SO2CI2]=0.12M,[CI2]=0.16M and [SO2]=0.050M. KC for the reaction is 0.078.Which of the systems described in Exercise 13.15 give homogeneous equilibria? Which give heterogeneous equilibria?Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?For which of the reactions in Exercise 13.15 does Kc (calculated using concentrations) equal KP (calculated using pressures)?For which of the reactions in Exercise 13.16 does Kc (calculated using concentrations) equal Kp (calculated using pressures)?Convert the values of KC to values of KP to the values of KP to values of Kc. (a) N2(g)+3H2(g)2NH3(g) Kc=0.50 at 400 C (b) H2(g)+I2(g)2HI(g) Kc=50.2 at 448 C (c) Na2SO410H2O(s)Na2SO4(s)+10H2O(g) Kp=4.081025 at 25C (d) H2O(l)H2O(g) Kp=0.122 at 50 C Covert the values of Kc to the values of KP or the values of Kp to values of Kc. (a) Cl2(g)+Br2(g)2BrCI(g) Kc=4.7102 at 25 C (b) 2SO2(g)+O2(g)2SO3(g) Kp=48.2 at 500 C (c) Ca2Cl26H2O(s)CaCl2(s)+6H2O(g) Kp=5.091044 at 25C (d) H2O(l)H2O(g) Kp=0.196 at 60 C What is the value of the equilibrium constant expression for the change H2O(l)H2O(g) at 30 C?Write the expression of the reaction quotient for the ionization of HOCN in water.Write the reaction quotient expression for the ionization of NH3 in water.What is the approximate value of the equilibrium constant KP for the change C2H5OC2H5(l)C2H5OC2H5(g) at 25 C. {Vapor pressure was described in the previous Chapter on liquids and solids; refer back to this chapter to find the relevant information needed to solve this problem.)The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?Explain how to recognize the conditions under which changes in pressure would affect systems at equilibrium.What property of a reaction can we use to predict the effect of a change in temperature on the value of an equilibrium constant?What would happen to the color of the solution in part (b) of Figure 13.8 if a small amount of NaOH were added and Fe(OH)3 precipitated? Explain your answer.The following reaction occurs when a burner on a gas stove is lit: CH4+2O2(g)CO2(g)+2H2O(g) Is an equilibrium among CH4, O2, CO2, and H2O established under these conditions? Explain your answer.A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide. SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO3 is higher, but the equilibrium amount (concentration or partial pressure) of SO3 is lower than it would be at lower temperatures. 2SO2(g)+O2(g)2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic?Suggest four ways in which the concentration of hydrazine, N2H4, could be increased in an equilibrium described by the following equation: N2(g)+2H2(g)N2H4(g)H=95kJ Suggest four ways in which the concentration of PH3could be increased in an equilibrium described by the following equation: P4(g)+6H2(g)4PH3(g)H=110.5kJ How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each? (a) 2NH3(g)N2(g)+3H2(g)H=92kJ (b) N2(g)+O2(g)2NO(g)H=181kJ (C) 2O3(g)3O2(g)H=585kJ (d) CaO(s)+CO2(g)CaCO3(s)H=176kJ How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each? (a) 2H2O(g)2H2(g)+O2(g)H=484kJ (b) N2(g)+3H2(g)2NH3(g)H=92.2kJ (c) 2Br(g)Br2(g)H=224kJ (d) H2(g)+I2(s)2HI(g)H=53kJ Water gas is a 1:1 mixture of carbon monoxide and hydrogen gas and is called water gas because it is formed from steam and hot carbon in the following reaction: H2O(g)+C(s)H2(g)+CO(g). Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and hydrogen at high temperature and pressure in the presence of a suitable catalyst. (a) Write the expression for the equilibrium constant (Kc) for the reversible reaction 2H2(g)+CO(g)CH3OH(g)H=90.2kJ (b) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more H2 is added? (c) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CO is removed? (d) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CH3OH is added? (e) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if the temperature of the system is increased? (f) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more catalyst is added?Nitrogen and oxygen react at high temperatures. (a) Write the expression for the equilibrium constant (Kc) for the reversible reaction N2(g)+O2(g)2NO(g)H=181kJ (b) What will happen to the concentrations of N2, O2, and NO at equilibrium if more O2 is added? (c) What will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed? (d) What will happen to the concentrations of N2, O2, and NO at equilibrium if NO is added? (e) What will happen to the concentrations of N2, O2, and NO at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel? (f) What will happen to the concentrations of N2, O2, and NO at equilibrium if the temperature of the system is increased? (g) What will happen to the concentrations of N2, O2, and NO at equilibrium if a catalyst is added?Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon. (a) Write the expression for the equilibrium constant for the reversible reaction C(s)+H2O(g)CO(g)+H2(g)H=131.30kJ (b) What will happen to the concentration of each reactant and product at equilibrium if more C is added? (c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed? (d) What will happen to the concentration of each reactant and product at equilibrium if CO is added? (e) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?Pure iron metal can be produced by the reduction of iron(III) oxide with hydrogen gas. (a) Write the expression for the equilibrium constant (Kc) for the reversible reaction Fe2O3(s)+3H2(g)2Fe(s)+3H2O(g)H=98.7kJ (b) What will happen to the concentration of each reactant and product at equilibrium if more Fe is added? (c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed? (d) What will happen to the concentration of each reactant and product at equilibrium if H2 is added? (e) What will happen to the concentration of each reactant and product at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel? (d) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?Ammonia is a weak base that reacts with water according to this equation: NH3(aq)+H2O(l)NH4+(aq)+OH(aq) Will any of the following increase the percent of ammonia that is converted to the ammonium ion in water? (a) Addition of NaOH (b) Addition of HCI (c) Addition of NH4CI Acetic acid is a weak acid that reacts with water according to this equation: CH3CO2H(aq)+H2O(aq)H3O+(aq)+CH3CO2(aq) Will any of the following increase the percent of acetic acid that reacts and produces CH3CO2 ion? (a) Addition of HCI (b) Addition of NaOH (c) Addition of NaCH3CO2 Suggest two ways in which the equilibrium concentration of Ag+ can be reduced in a solution of Na+, Cl-, Ag+, and NO3-, in contact with solid AgCl. Na+(aq)+CI(aq)+Ag+(aq)+NO3(aq)AgCI(s)+Na+(aq)+NO3(aq)H=65.9kJ How can the pressure of water vapor be increased in the following equilibrium? H2O(l)H2O(g)H=41kJ Additional solid silver sulfate, a slightly soluble solid, is added to a solution of silver ion and sulfate ion at equilibrium with solid silver sulfate. 2Ag++SO42(aq)Ag2SO4(s) Which of the following will occur? (a) Ag+ or SO42- concentrations will not change. (b) The added silver sulfate will dissolve. (c) Additional silver sulfate will form and precipitate from solution as Ag+ ions and SO42- ions combine. (d) The Ag+ ion concentration will increase and the SO42- ion concentration will decrease.The amino acid alanine has two isomers, -alanine and -alanine. When equal masses of these two compounds are dissolved in equal amounts of a solvent, the solution of -alanine freezes at the lowest temperature. Which form, -alanine or -alanine, has the larger equilibrium constant for ionization (HXH++X)?A reaction is represented by this equation: A(aq)+2B2C(aq) Kc=1103 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations M, make up two sets of concentrations that describe a mixture of A, B, and C at equilibrium.A reaction is represented by this equation: 2W(aq)X(aq)+2Y(aq)Kc=5104 (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations of M, make up [we sets of concentrations that describe a mixture of W, X, and Y at equilibrium.What is the value of the equilibrium constant at 500 C for the formation of NH3 according to the following equation? N2(g)+3H2(g)2NH3(g) An equilibrium mixture of NH3(g), H2(g), and N2(g) at 500 C was found to contain 1.35 M H2, 1.15 M N2, and 4.12101M NH3.Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4(g)+H2O(g)3H2(g)+CO(g) What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M ; H2O, 0.242 M ; CO, 0.126 M ; H2 1.15 M, at a temperature of 760 C?A 0.72-m01 sample of PCl5 is put into a 1.00-L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCl3(g ) and 0.40 mol of Cl2(g). Calculate the value of the equilibrium constant for the decomposition of PCl5 to PCl3 and Cl2 at this temperature.At 1 atm and 25 C, NO2 with an initial concentration of 1.00 M is 3.3103 decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction. 2NO2(g)2NO(g)+O2(g)Calculate the value of the equilibrium constant Kp for the reaction 2NO2(g)+Cl2(g)2NOCl(g) from these equilibrium pressures: NO, 0.050 atm; Cl2, 0.30 arm; NOCI, 1.2 mm.When heated, iodine vapor dissociates according to this equation: I2(g)2I(g) At 1274 K, a sample exhibits a partial pressure of I2 of 0.1122 atm and a partial pressure due to I atoms of 0.1378 atm. Determine the value of the equilibrium constant, Kp, for the decomposition at 1274 K.A sample of ammonium chloride was heated in a closed container. NH4CI(s)NH3(g)+HCI(g) At equilibrium, the pressure of NH3(g) was found to be 1.75 atm. What is the value of the equilibrium constant KP for the decomposition at this temperature?At a temperature of 60 C, the vapor pressure of water is 0.196 atm. What is the value of the equilibrium constant KP for the transformation at 60 C? H2O(l)H2O(g)Complete the changes in concentrations (or pressure, if requested) for each of the following reactions. (a) 2SO3(g)2SO2+O2(g) + x 0.125 M (b) 4NH3(g)+3O2(g)2N2(g)+6H2O(g) 3x 0.24 M (c) Change in pressure: 2CH4(g)C2H2(g)+3H2(g) x 25 torr (d) Change in pressure: CH4(g)+H2O(g)CO(g)+3H2(g) x 5 atm (e) CH4CI(s)NH3(g)+HCI(g) x 1.03104 M (e) Change in pressure: Ni(s)+4CO(g)Ni(CO)4(g) 4x 0.40 atm Complete the changes in concentrations (or pressure, if requested) for each of the following reactions‘ (a) 2H2(g)+O2(g)2H2O(g) + 2x 1.50M (b) CS2(g)+4H2(g)CH4(g)+2H2S(g) x 0.020 M (c) Change in pressure: H2(g)+CI2(g)2HCI(g)x 1.50 atm (d) Change in pressure: 2NH3(g)+2O2(g)N2O(g)+3H2O(g) x = 60.6 torr (e) NH4HS(s)NH3+H2S(g) x 9.8106M (f) Change in pressure: Fe(s)+5CO(g)Fe(CO)5(g) x 0.012 atm Why are there no changes specified for Ni in Exercise 13.61, part (f)? What property of Ni does change?Why are there no changes specified for NH4HS in Exercise 13.62, part (e)? What property of NH4HS does change?Analysis of the gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at 400 C established the concentration of N2 to be 1.2 M and the concentration of H2 to be 0.24 M. N2(g)+3H2(g)2NH3(g)Kc=0.50 at 400 C Calculate the equilibrium molar concentration of NH3.Calculate the number of moles of HI that are at equilibrium with 1.25 mol of H2 and 1.25 mol of I2 in a 5.00-L flask at 44 C. H2+I22HI at Kc=50.2 at 448 C What is the pressure of BrCl in an equilibrium mixture of Cl2, Br2, and BrCl if the pressure of CI2 in the mixture is 0.115 atm and the pressure of Br2 in the mixture is 0.450 atm? Cl2(g)+Br2(g)2BrCl(g)KP=4.7102 What is the pressure of CO2 in a mixture at equilibrium that contains 0.50 mm H2, 2.0 atm of H2O, and 1.0 mm of CO at 990 C? H2(g)+CO2(g)H2O(g)+CO(g)KP=1.6 at 990 C Cobalt metal can be prepared by reducing cobalt (II) oxide with carbon monoxide. CoO(s)+CO(g)Co(s)+CO2(g)Kc=4.90102 at 550 C Carbon reacts with water vapor at elevated temperatures. C(s)+H2O(g)Co(g)+H2(g)Kc=0.2 at 1000 C What is the concentration of CO in an equilibrium mixture with [H2O]=0.500M at 1000 C?Sodium sulfate 10-hydrate, Na2SO410H2O, dehydrates according to the equation Na2SO410H2O(s)Na2SO4(s)+10H2O(g)KP=4.081025 at 25 C What is the pressure of water vapor at equilibrium with a mixture of Na2SO410H2O and NaSO4?Calcium Chloride 6-hydrate, CaCl26H2O, dehydrates according to the equation CaCl26H2O(s)CaCl2(s)+6H2O(g)KP=5.091044 at 25 C What is the pressure of water vapor at equilibrium with a mixture of CaCl26H2O and CaCl2?A student solved the following problem and found the equilibrium concentrations to be [SO2]=0.590M,[O2]=0.0450M, and [SO3]=0.260M. How could this student check the work without reworking the problem? The problem was: For the following reaction at 600 C: 2SO2(g)+O2(g)2SO3(g)Kc=4.32 A student solved the following problem and found [N2O4]=0.16M at equilibrium. How could this student recognize that the answer was wrong without reworking the problem? The problem was: What is the equilibrium concentration of N2O4 in a mixture formed from a sample of NO2 with a concentration of 0.10 M? 2NO2(g)N2O4(g)Kc=160 Assume that the change in concentration of N2O4 is small enough to be neglected in the following problem (a) Calculate the equilibrium concentration of both species in 1.00 L of a solution prepared from 0.129 mol of N2O4 with chloroform as the solvent. N2O4(g)2O2(g)Kc=1.07105 in chloroform (b) Show that the change is small enough to be neglected.Assume that the change in concentration of COCI2 is small enough to be neglected in the following problem. (a) Calculate the equilibrium concentration of all species in an equilibrium mixture that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCI2(g)CO(g)+CI2(g)Kc=2.21010 (b) Show that the change is small enough to be neglected.Assume that the change in pressure of H2S is small enough to be neglected in the following problem, (a) Calculate the equilibrium pressures of all species in an equilibrium mixture that results from the decomposition of H2S with an initial pressure of 0.824 atm. 2H2S(g)2H2(g)+S2(g)Kp=2.2106 (b) Show that the change is small enough to be neglected.What are all concentrations after a mixture that contains [H2O]=1.00M and [Cl2O]=1.00M comes to equilibrium at 25 C? H2O(g)+Cl2O(g)2HOCl(g)Kc=0.0900 What are the concentrations of PCl5, PCl3, and Cl2 in an equilibrium mixture produced by the decomposition of a sample of pure PCI5 with [PCl5]=2.00M? PCl5(g)PCl3(g)+Cl2(g)Kc=0.0211 Calculate the pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2 produced when a sample of NOCl with a pressure of 10.0 atm comes to equilibrium according to this reaction: 2NOCl(g)2NO(g)+Cl2(g)Kp=4.0104 Calculate the equilibrium concentrations of NO, O2, and NO2 in a mixture at 250 C that results from the reaction of 0.20 M NO and 0.10 M O2. (Hint: K is large; assume the reaction goes to completion then comes back to equilibrium.) 2NO(g)+O2(g)2NO2(g)Kc=2.3105 at 25 C Calculate the equilibrium concentrations that result when 0.25 M O2 and 1.0 M HCl react and come to equilibrium. 4HCl(g)+O2(g)2Cl2+2H2O(g)Kc=3.11013 One of the important reactions in the formation of smog is represented by the equation O3(g)+NO(g)NO2(g)+O2(g)Kp=6.01034 What is the pressure of O3 remaining after a mixture of O3 with a pressure of 1.2108 arm and NO with a pressure of 1.2108 atm comes to equilibrium? (Hint: KP is large; assume the reaction goes to completion then comes back to equilibrium.)Calculate the pressures of NO, Cl2, and NOCI in an equilibrium mixture produced by the reaction of a starting mixture with 4.0 atm NO and 2.0 atm Cl2. (Hint: KP is small; assume the reverse reaction goes to completion then comes back to equilibrium.) 2NO(g)+Cl(g)2NOCl(g)Kp=2.5103 Calculate the number of grams of HI that are at equilibrium with 1.25 mol of H2 and 63.5 g of iodine at 448 C. H2+I22HIKc=50.2 at 448 C Butane exists as two isomers, n -butane and isobutane. Kp=2.5 at 25 C What is the pressure of isobutane in a container of the two isomers at equilibrium with a total pressure of 1.22 am?What is the minimum mass of CaCO3 required to establish equilibrium at a certain temperature in a 6.50-L container if the equilibrium constant (Kc) is 0.050 for the decomposition reaction of CaCO3 at that temperature? CaCO3(s)CaO(s)+CO2(g)The equilibrium constant (Kc) for this reaction is 1.60 at 990 c: H2(g)+CO2(g)H2O(g)+CO(g) Calculate the number of moles of each component in the final equilibrium mixture obtained from adding 1.00 mol of H2, 2.00 mol of CO2, 0.750 mol of H2O, and 1.00 mol of CO to a 5.00-L container at 990 c.At 25 C and at 1 atm, the partial pressures in an equilibrium mixture of N2O4 and NO2 are PN2O4=0.70 atm and PNO2=0.30 atm. (a) Predict how the pressures of NO2 and N2O4 will change if the total pressure increases to 9.0 atm. Will they increase, decrease, or remain the same? (b) Calculate the partial pressures of NO2 and N2O4 when they are at equilibrium at 9.0 atm and 25 C.In a 3.0-L vessel, the following equilibrium partial pressures are measured: N2, 190 torr; H2, 317 torr; NH3, 1.00103 torr. N2(g)+3H2(g)2NH3(g) (a) How will the partial pressures of H2, N2, and NH3 change if H2 is removed from the system? Will they increase, decrease, or remain the same? (b) Hydrogen is removed from the vessel until the partial pressure of nitrogen, at equilibrium, is 250 torr. Calculate the partial pressures of the other substances under the new conditions.The equilibrium constant (Kc) for this reaction is 5.0 at a given temperature. CO(g)+H2O(g)CO2(g)+H2(g) (a) On analysis, an equilibrium mixture of the substances present at the given temperature was found to contain 0.20 mol of CO, 0.30 mol of water vapor, and 0.90 mol of H2 in a liter. How many moles of CO2 were there in the equilibrium mixture? (b) Maintaining the same temperature, additional H2 was added to the system, and some water vapor was removed by drying. A new equilibrium mixture was thereby established containing 0.40 mol of CO, 0.30 mol of water vapor, and 1.2 mol of H2 in a liter. How many moles of CO2 were in the new equilibrium mixture? Compare this with the quantity in part (a), and discuss whether the second value is reasonable. Explain how it is possible for the water vapor concentration to be the same in the two equilibrium solutions even though some vapor was removed before the second equilibrium was established.Antimony pentachloride decomposes according to this equation: SbCl5(g)SbCl3+Cl2(g) An equilibrium mixture in a 5.00-L flask at 443 C contains 3.85 g of SbCl5, 9.14 g of SbCl3, and 2.84 g of Cl2. How many grams of each will be found if the mixture is transferred into a 2.00-L flask at the same temperature?Consider the reaction between H2 and O2 at 1000 2H2(g)+O22H2O(g)Kp=( P H 2 O )2(P o2 )( P H 2 )2=1.331020 If 0.500 atm of H2 and 0.500 arm of O2 are allowed to come to equilibrium at this temperature, what are the partial pressures of the components?An equilibrium is established according to the following equation Hg22+(aq)+NO3(aq)+3H+(aq)2Hg2+(aq)+HNO2(aq)+H2O(l)Kc=4.6 What will happen in a solution that is 0.20 M each in Hg22+, NO3-, H+, Hg2+, and HNO2? (a) Hg22+ will be oxidized and NO3- reduced. (b) Hg22+ will be reduced and NO3- oxidized. (c) Hg22+ will be oxidized and HNO2 reduced. (d) Hg22+ will be reduced and HNO2 oxidized. (e) There will be no change because all reactants and products have an activity of 1.Consider the equilibrium 4NO2(g)+6H2O(g)4NH3(g)+7O2(g) (a) What is the expression for the equilibrium constant (Kc) of the reaction? (b) How must the concentration of NH3 change to reach equilibrium if the reaction quotient is less than the equilibrium constant? (c) If the reaction were at equilibrium, how would a decrease in pressure (from an increase in the volume of the reaction vessel) affect the pressure of NO2? (d) If the change in the pressure of NO2 is 28 torr as a mixture 0f the four gases reaches equilibrium, how much will the pressure of O2 change?The binding of oxygen by hemoglobin (Hb), giving oxy-hemoglobin (HbO2), is partially regulated by the concentration of H3O+ and dissolved CO2 in the blood. Although the equilibrium is complicated, it can be summarized as HbO2(aq)+H3O+(aq)+CO2(g)CO2HbH++O2(g)+H2O(l) (a) Write the equilibrium constant expression for this reaction. (b) Explain why the production of lactic acid and CO2 in a muscle during exertion stimulates release of O2 from the oxy-hemoglobin in the blood passing through the muscle.The hydrolysis of the sugar sucrose to the sugars glucose and fructose follows a first-order rate equation for the disappearance of sucrose. C12H22O11(aq)+H2O(l)C6H12O6(aq)+C6H12O6(aq) Rate =k[C12H22O11] In neutral solution, k=2.11011 at 27 C. (As indicated by the rate constant, this is a very slow reaction. In the human body, the rate of this reaction is sped up by a type of catalyst called an enzyme.) (Note: That is not a mistake in the equation—the products of the reaction, glucose and fructose, have the same molecular formulas, C6H12O6, but differ in the arrangement of the atoms in their molecules). The equilibrium constant for the reaction is 1.36105 at 27 C. What are the concentrations of glucose, fructose, and sucrose after a 0.150 M aqueous solution of sucrose has reached equilibrium? Remember that the activity of a solvent (the effective concentration) is 1.The density of trifluoroacetic acid vapor was determined at 118.1 C and 468.5 torr, and found to be 2.784 g/L. Calculate KC for the association of the acid.Liquid N2o3 is dark blue at low temperatures, but the color fades and becomes greenish at higher temperatures as the compound decomposes to NO and NO2. At 25 C, a value of Kp=1.91 has been established for this decomposition. If 0.236 moles of N2O3 are placed in a 1.52-L vessel at 25 C, calculate the equilibrium partial pressures of N2O3(g), No2(g), and NO(g).A 1.00-L vessel at 400 C contains the following equilibrium concentrations: N2, 1.00 M; H2, 0.50 M; and NH3, 0.25 M. How many moles of hydrogen must be removed from the vessel to increase the concentration of nitrogen to 1.1 M?A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 C. A 0.010 M solution of the weak acid HB has an osmotic pressure of 0.345 atm under the same conditions. (a) Which acid has the larger equilibrium constant for ionization HA[HA(aq)A(aq)+H+(aq)] or HB[HB(aq)H+(aq)+B(aq)]? (b) What are the equilibrium constants for the ionization of these acids? (Hint: Remember that each solution contains three dissolved species: the weak acid (HA or HB). the conjugate base (A- or B- and the hydrogen ion (H+). Remember that osmotic pressure (like all colligative properties) is related to the total number of solute particles. Specifically for osmotic pressure, those concentrations are described by molarities.)Write equations that show NH3 as both a conjugate acid and a conjugate base.Write equations that show H2PO4- acting both as an acid and as a base.Show by suitable net ionic equations that each of the following species can act as a Br usted-Lowry acid: (a) H3O+. (b) HCl. (c) NH3. (d) CH3CO2H. (e) NH4+. (f) HSO4-Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry acid: (a) HNO3. (b) PH4+. (c) H25. (d) CH3CH2COOH. (e) H2PO4-. (f) HS-Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry base: (a) H2O. (b) OH-. (c) NH3. (d) CN-. (e) S2-. (f) H2PO4-Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry base: (a) HS-. (b) PO43-. (C) NH2-. (d) C2H5OH. (e) O2-. (f) H2PO4-What is the conjugate acid of each of the following? What is the conjugate base of each?. (a) OH-. (b) H2O. (c) HCO3-. (d) NH3. (e) HSO4-. (f) H2O2. (g) HS-. (h) H5N2+What is the conjugate acid of each of the following? What is the conjugate base of each?. (a) H2S. (b) H2 PO4-. (c) PH3. (d) HS-. (e) HSO3-. (f) H3O2+. (g) H4N2. (h) CH3OH Identify and label the Bronsted-Lowry acid, its conjugate base, the Bronsted—Lowry base, and its conjugate acid in each of the following equations: (a) HNO3+H2OH3O++NO3 (b) CN+H2OHCN+OH (c) H2SO4+CIHCI+HSO4 (d) HSO4+OHSO42+H2O (e) O2+H2O2OH (f) [Cu( H 2 O)3(OH)]++[Al( H 2 O)6]3+[Cu( H 2 O)4]2++[Al( H 2 O)5(OH)]2+ (g) H2S+NH2HS+NH3 Identify and label the Bronsted-Lowry acid, its conjugate base, the Bronsted-Lowry base, and its conjugate acid in each of the following equations: (a) NO2+H2OHNO2+OH (b) HBR+H2OH3O++Br (c) HS-+H2OH2S+OH (d) H2PO4+OHHPO42+H2O (e) H2PO4+HClH3PO4+Cl (f) [Fe( H 2 O)5(OH)]2++[Al( H 2 O)6]3+[Fe( H 2 O)6]3++[Al( H 2 O)5(OH)]2+ (g) CH3OH+HCH3O+H2 What are amphiprotic species? Illustrate with suitable equations.State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species: (a) H2O. (b) H2PO4-. (c) S2-. (d) CO32-. (e) HSO4-State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species. (a) NH3. (b) HPO4-. (c) Br-. (d) NH4+. (e) ASO43-Is the self-ionization of water endothermic or exothermic? The ionization constant for water (Kw) is 2.91014 at 40 C and 9.31014 at 60 C.Explain why a sample of pure water at 40 C is neutral even though [H3O+]=1.7107M . Kw is 2.91014 at 40 C.The ionization constant for water (Kw) is 2.91014 at 40 C. Calculate [H3O+], [OH-], pH, and pOH for pure water at 40 C.The ionization constant for water (Kw) is 9.3111014 at 60 C. Calculate [H3O+], [OH-], pH, and pOH for pure water at 60 C.Calculate the pH and the pOH of each of the following solutions at 25 C for which the substances ionize completely: (a) 0.200 M HCl. (b) 0.0143 M NaOH. (c) 3.0 M HNO3. (d) 0.0031 M Ca(OH)2 Calculate the pH and the pOH of each of the following solutions at 25 C for which the substances ionize completely: (a) 0.000259 M HClO4. (b) 0.21 M NaOH. (c) 0.000071 M Ba(OH)2. (d) 2.5 M KOH What are the pH and pOH of a solution of 2.0 M HCl, which ionizes completely?What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52?Calculate the hydrogen ion concentration and the hydroxide ion concentration in wine from its pH, See Figure 14.2 for useful information.Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice from its pH, See Figure 14.2 for useful information.The hydronium ion concentration in a sample of rainwater is found to be 1.7106M at 25 C. What is the concentration of hydroxide ions in the rainwater?The hydroxide ion concentration in household ammonia is 3.2103M at 25 C. What is the concentration of hydronium ions in the solution?Explain why the neutralization reaction of a strong acid and a weak base gives a weakly acidic solution.Explain why the neutralization reaction of a weak acid and a strong base gives a weakly basic solution.Use this list of important industrial compounds (and Figure 14.8) to answer the following questions regarding: CaO, Ca(OH)2, CH3CO2H, CO2, HCl, H2CO3, HF, HNO2, HNO3, H3PO4, H2SO4, NH3, NaOH, Na2CO3. (a) Identify the strong Bronsted-Lowry acids and strong Bronsted-Lowry bases. (b) List those compounds in (a) that can behave as Bronsted-Lowry acids with strengths lying between those of H3O+ and H2O. (c) List those compounds in (a) that can behave as Bronsted-Lowry bases with strengths lying between those of H2O and OH-.The odor of vinegar is due to the presence of acetic acid, CH3CO2H, a weak acid. List, in order of descending concentration, all of the ionic and molecular species present in a 1-M aqueous solution of this acid.Household ammonia is a solution of the weak base NH3 in water. List, in order of descending concentration, all of the ionic and molecular species present in a1-M aqueous solution of this base.Explain why the ionization constant, Ka, for H2SO4 is larger than the ionization constant for H2SO3.Explain why the ionization constant, Ka, for HI is larger than the ionization constant for HP.Gastric juice, the digestive ?uid produced in the stomach, contains hydrochloric acid, HCl, Milk of Magnesia, a suspension of solid Mg(OH)2 in an aqueous medium, is sometimes used to neutralize-excess stomach acid. Write a complete balanced equation for the neutralization reaction, and identify the conjugate acid—base pairs.Nitric acid reacts with insoluble copper (II) oxide to form soluble copper (II) nitrate, Cu(NO3)2, a compound that has been used to prevent the growth of algae in swimming pools. Write the balanced chemical equation for the reaction of an aqueous solution of HNO3 with CuO.What is the ionization constant at 25 C for the weak acid CH3 NH3+, the conjugate acid of the weak base CH3NH2, Kb=4.4104.What is the ionization constant at 25 C for the weak acid (CH3)2 NH2+, the conjugate acid of the weak base (CH3)2NH, Kb=5.9104?Which base, CH3NH2 or (CH3)2NH, is the stronger base? Which conjugate acid, (CH3)2NH2+ or (CH3)2NH3+, is the stronger acid?Which is the stronger acid, NH4+ or HBrO?Which is the stronger base, (CH3)3N or H2BO3-?Predict which acid in each of the following pairs is the stronger and explain your reasoning for each.. (a) H2O or HF. (b) B(OH)3 or Al(OH)3. (c) HSO3- or HSO4-. (d) NH3 or H2S. (e) H2O or H2Te Predict which compound in each of the following pairs of compounds is more acidic and explain your reasoning for each. (a) HSO4- or HSeO4-. (b) NH3 or H2O. (c) PH3 or HI. (d) NH3 or PH3. (e) H2S or HBr Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: HCI, HBr, HI. (b)basicity: H2O, OH-, H-, CI-. (c) basicity: Mg(OH)2, Si(OH)4, ClO3(OH) (Hint: Formula could also be written as HCIO4). (d) acidity: HF, H2O, NH3, CH4 Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: NaHSO3, NaHSeO3, NaHSO4. (b) basicity: BrO2-, ClO2-,IO2-. (c) acidity: HOCI, HOBr, HOI. (d) acidity: HOCl, HOClO, HOClO2, HOClO3. (e) basicity: NH2-, HS-, HTe-, PH2-. (f) basicity: BrO-, BrO2-, Bro3-, BrO4-Both HF and HCN ionize in water to a limited extent. Which of the conjugate bases. F“ or CN”, is the stronger base? See Table 14.2.The active ingredient formed by aspirin in the body is salicylic acid, C6H4OH(CO2H). The carboxyl group. (-CO2H) acts as a weak acid. The phenol group (an OH group bonded to an aromatic ring) also acts as an acid but a much weaker acid. List, in order of descending concentration, all of the ionic and molecular species present in a 0.001-M aqueous solution of C6H4OH(CO2H).What do we represent when we write: CH3CO2H(aq)+H2O(l)H3O+(aq)+CH3CO2(aq)?Explain why equilibrium calculations are not necessary to determine ionic concentrations in solutions of certain strung electrolytes such as NaOH and HCl. Under what conditions are equilibrium calculations necessary as part of the determination of the concentrations of all ions of some other strong electrolytes in solution?Are the concentrations of hydronium ion and hydroxide ion in a solution of an acid or a base in water directly proportional or inversely proportional? Explain your answer.What two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak acid?What two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak base?Which of the following will increase the percent of NH3 that is converted to the ammonium ion in water (Hint: Use LeChatelier’s principle.)? (a) addition of NaOH. (b) addition of HCl. (c) addition of NH4Cl Which of the following will increase the percent of HF that is converted to the fluoride ion in water?. (a) addition of NaOH. (b) addition of HCl. (c) addition of NaF What is the effect on the concentrations of NO2-, HNO2, and OH- when the following are added to a solution of KNO2 in water: (a) HCl. (b) HNO2. (c) NaOH. (d) NaCl. (e) KNO The equation for the equilibrium is: NO2(aq)+H2O(l)HNO2+OH(aq)What is the effect on the concentration of hydro?uoric acid, hydronium ion, and fluoride ion when the following are added to separate solutions of hydrofluoric acid? (a) HCl. (b) KF. (c) NaCl. (d) KOH. (e) HF The equation for the equilibrium is: HF(aq)+H2O(l)H3O+(aq)+F(aq)Why is the hydronium ion concentration in a solution that is 0.10 M in HCl and 0.10 M in HCOOH determined by the concentration of HCl?From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb, for each of the weak bases. (a). CH3CO2H:[H3O+]=1.34103M;[CH3CO2]=1.34103M;[CH3CO2H]=9.866102M; (b). ClO:[OH]=4.0104M;[HClO]=2.38105M;[ClO]=0.273M; (c). HCO2H:[HCO2H]=0.524M;[H3O+]=9.8103M;[HCO2]=9.8103M; (d). C6H5NH3+:[C6H5NH3+]=0.233M;[C6H5NH2]=2.3103M;[H3O+]=2.3103M

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