Chemistry 9th Edition
ISBN: 9781133611097
Author: Steven S. Zumdahl
Publisher: Steven S. Zumdahl
1 Chemical Foundations 2 Atoms, Molecules, And Ions 3 Stoichiometry 4 Types Of Chemical Reactions And Solution Stoichiometry 5 Gases 6 Thermochemistry 7 Atomic Structure And Periodicity 8 Bonding: General Concepts 9 Covalent Bonding: Orbitals 10 Liquids And Solids 11 Properties Of Solutions 12 Chemical Kinetics 13 Chemical Equilibrium 14 Acids And Bases 15 Acid-base Equilibria 16 Solubility And Complex Ion Equilibria 17 Spontaneity, Entropy, And Free Energy 18 Electrochemistry 19 The Nucleus: A Chemist's View 20 The Representative Elements 21 Transition Metals And Coordination Chemistry 22 Organic And Biological Molecules Chapter15: Acid-base Equilibria
Chapter Questions Section: Chapter Questions
Problem 1RQ: What is meant by the presence of a common ion? How does the presence of a common ion affect an... Problem 2RQ: Define a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with... Problem 3RQ: One of the most challenging parts of solving acidbase problems is writing out the correct equation.... Problem 4RQ: A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If... Problem 5RQ: Draw the general titration curve for a strong acid titrated by a strong base. At the various points... Problem 6RQ: Instead of the titration of a strong acid by a strong base considered in Question 5, consider the... Problem 7RQ: Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations... Problem 8RQ: Sketch the titration curve for a weak base titrated by a strong acid. Weak basestrong acid titration... Problem 9RQ: What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a... Problem 10RQ: Why does an indicator change from its acid color to its base color over a range of pH values? In... Problem 1ALQ: What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of... Problem 2ALQ: A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt... Problem 3ALQ: Mixing together solutions of acetic acid and sodium hydroxide can make a buffered solution. Explain.... Problem 4ALQ: Could a buffered solution be made by mixing aqueous solutions of HCl and NaOH? Explain. Why isnt a... Problem 5ALQ: Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong... Problem 6ALQ: Sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH). List the major... Problem 7ALQ: You have a solution of the weak acid HA and add some HCl to it. What are the major species in the... Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major... Problem 9Q: The common ion effect for weak acids is to significantly decrease the dissociation of the acid in... Problem 10Q Problem 11Q: A best buffer has about equal quantities of weak acid and conjugate base present as well as having a... Problem 12Q: Consider the following pH curves for 100.0 mL of two different acids with the same initial... Problem 13Q: An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker... Problem 14Q: Consider the following four titrations. i. 100.0 mL of 0.10 M HCl titrated by 0.10 M NaOH ii. 100.0... Problem 15Q: Figure 14-4 shows the pH curves for the titrations of six different acids by NaOH. Make a similar... Problem 16Q: Acidbase indicators mark the end point of titrations by magically turning a different color. Explain... Problem 17E: How many of the following are buffered solutions? Explain your answer. Note: Counter-ions and water... Problem 18E: Which of the following can be classified as buffer solutions? a. 0.25 M HBr + 0.25 M HOBr b. 0.15 M... Problem 19E: A certain buffer is made by dissolving NaHCO3 and Na2CO3 in some water. Write equations to show how... Problem 20E: A buffer is prepared by dissolving HONH2 and HONH3NO3 in some water. Write equations to show how... Problem 21E: Calculate the pH of each of the following solutions. a. 0.100 M propanoic acid (HC3H5O2, Ka = 1.3 ... Problem 22E: Calculate the pH of each of the following solutions. a. 0.100 M HONH2 (Kb= 1.1 108) b. 0.100 M... Problem 23E: Compare the percent dissociation of the acid in Exercise 21a with the percent dissociation of the... Problem 24E: Compare the percent ionization of the base in Exercise 22a with the percent ionization of the base... Problem 25E: Calculate the pH after 0.020 mole of HCl is added to 1.00 L of each of the four solutions in... Problem 26E: Calculate the pH after 0.020 mole of HCl is added to 1.00 L of each of the four solutions in... Problem 27E: Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of each of the four solutions in... Problem 28E: Calculate the pH after 0.020 mole of NaOH is added to 1.00 L of each of the solutions in Exercise... Problem 29E: Which of the solutions in Exercise 21 shows the least change in pH upon the addition of acid or... Problem 30E Problem 31E: Calculate the pH of a solution that is 1.00 M HNO2 and 1.00 M NaNO2. Problem 32E: Calculate the pH of a solution that is 0.60 M HF and 1.00 M KF. Problem 33E: Calculate the pH after 0.10 mole of NaOH is added to 1.00 L of the solution in Exercise 31, and... Problem 34E: Calculate the pH after 0.10 mole of NaOH is added to 1.00 L of the solution in Exercise 32, and... Problem 35E: Calculate the pH of each of the following buffered solutions. a. 0.10 M acetic acid/0.25 M sodium... Problem 36E: Calculate the pH of each of the following buffered solutions. a. 0.50 M C2H5NH2/0.25 M C2H5NH3Cl b.... Problem 37E: Calculate the pH of a buffered solution prepared by dissolving 21.5 g benzoic acid (HC7H5O2) and... Problem 38E: A buffered solution is made by adding 50.0 g NH4Cl to 1.00 L of a 0.75-M solution of NH3. Calculate... Problem 39E: Calculate the pH after 0.010 mole of gaseous HCl is added to 250.0 mL of each of the following... Problem 40E: An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 M... Problem 41E: Calculate the mass of sodium acetate that must be added to 500.0 mL of 0.200 M acetic acid to form a... Problem 42E: What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered... Problem 43E: Consider a solution that contains both C5H5N and C5H5NHNO3. Calculate the ratio [C5H5N]/[C5H5NH+] if... Problem 44E: Calculate the ratio [NH3]/[NH4+] in ammonia/ammonium chloride buffered solutions with the following... Problem 45E: Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid... Problem 46E: When a person exercises, muscle contractions produce lactic acid. Moderate increases in lactic acid... Problem 47E: Consider the acids in Table 13-2. Which acid would be the best choice for preparing a pH = 7.00... Problem 48E: Consider the bases in Table 13-3. Which base would be the best choice for preparing a pH = 5.00... Problem 49E: Calculate the pH of a solution that is 0.40 M H2NNH2 and 0.80 M H2NNH3NO3. In order for this buffer... Problem 50E: Calculate the pH of a solution that is 0.20 M HOCl and 0.90 M KOCl. In order for this buffer to have... Problem 51E: Which of the following mixtures would result in buffered solutions when 1.0 L of each of the two... Problem 52E: Which of the following mixtures would result in a buffered solution when 1.0 L of each of the two... Problem 53E: What quantity (moles) of NaOH must be added to 1.0 L of 2.0 M HC2H3O2 to produce a solution buffered... Problem 54E: Calculate the number of moles of HCl(g) that must be added to 1.0 L of 1.0 M NaC2H3O2 to produce a... Problem 55E: Consider the titration of a generic weak acid HA with a strong base that gives the following... Problem 56E: Sketch the titration curve for the titration of a generic weak base B with a strong acid. The... Problem 57E: Consider the titration of 40.0 mL of 0.200 M HClO4 by 0.100 M KOH. Calculate the pH of the resulting... Problem 58E: Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the... Problem 59E: Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate... Problem 60E: Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 106) by 0.200 M HNO3. Calculate the... Problem 61E: Lactic acid is a common by-product of cellular respiration and is often said to cause the burn... Problem 62E: Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M propanoic acid... Problem 63E: Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M NH3 (Kb = 1.8 105)... Problem 64E: Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100... Problem 65E: Calculate the pH at the halfway point and at the equivalence point for each of the following... Problem 66E: In the titration of 50.0 mL of 1.0 M methylamine, CH3NH2 (Kb = 4.4 104), with 0.50 M HC1, calculate... Problem 67E: You have 75.0 mL of 0.10 M HA. After adding 30.0 mL 0.10 M NaOH, the pH is 5.50. What is the Ka... Problem 68E: A student dissolves 0.0100 mole of an unknown weak base in 100.0 mL water and titrates the solution... Problem 69E: Two drops of indicator HIn (Ka = 1.0 109), where HIn is yellow and In is blue, are placed in 100.0... Problem 70E: Methyl red has the following structure: It undergoes a color change from red to yellow as a solution... Problem 71E: Potassium hydrogen phthalate, known as KHP (molar mass = 204.22 g/mol), can be obtained in high... Problem 72E: A certain indicator HIn has a pKa of 3.00 and a color change becomes visible when 7.00% of the... Problem 73E: Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 57 and 59? Problem 74E Problem 75E: Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63? Problem 76E Problem 77E: Estimate the pH of a solution in which bromcresol green is blue and thymol blue is yellow. (See Fig.... Problem 78E: Estimate the pH of a solution in which crystal violet is yellow and methyl orange is red. (See Fig.... Problem 79E: A solution has a pH of 7.0. What would be the color of the solution if each of the following... Problem 80E: A solution has a pH of 4.5. What would be the color of the solution if each of the following... Problem 81AE: Derive an equation analogous to the HendersonHasselbalch equation but relating pOH and pKb of a... Problem 82AE: a. Calculate the pH of a buffered solution that is 0.100 M in C6H5CO2H (benzoic acid, Ka = 6.4 105)... Problem 83AE: Tris(hydroxymethyl)aminomethane, commonly called TRIS or Trizma, is often used as a buffer in... Problem 84AE: You make 1.00 L of a buffered solution (pH = 4.00) by mixing acetic acid and sodium acetate. You... Problem 85AE: You have the following reagents on hand: Solids (pKa of Acid Form Is Given) Solutions Benzoic acid... Problem 86AE Problem 87AE: Phosphate buffers are important in regulating the pH of intracellular fluids at pH values generally... Problem 88AE: What quantity (moles) of HCl(g) must be added to 1.0 L of 2.0 M NaOH to achieve a pH of 0.00?... Problem 89AE Problem 90AE: The following plot shows the pH curves for the titrations of various acids by 0.10 M NaOH (all of... Problem 91AE: Calculate the volume of 1.50 102 M NaOH that must be added to 500.0 mL of 0.200 M HCl to give a... Problem 92AE Problem 93AE: A certain acetic acid solution has pH = 2.68. Calculate the volume of 0.0975 M KOH required to reach... Problem 94AE: A 0.210-g sample of an acid (molar mass = 192 g/mol) is titrated with 30.5 mL of 0.108 M NaOH to a... Problem 95AE: The active ingredient in aspirin is acetylsalicylic acid. A 2.51-g sample of acetylsalicylic acid... Problem 96AE: One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and... Problem 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution... Problem 98AE: A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein end point with 25.0 mL... Problem 99AE: A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.125 M NaOH,... Problem 100CWP: Consider 1.0 L of a solution that is 0.85 M HOC6H5 and 0.80 M NaOC6H5. (Ka for HOC6H5 = 1.6 1010.)... Problem 101CWP: What concentration of NH4Cl is necessary to buffer a 0.52-M NH3 solution at pH= 9.00? (Kb for NH3 =... Problem 102CWP: Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 ... Problem 103CWP: Consider a buffered solution containing CH3NH3Cl and CH3NH2. Which of the following statements... Problem 104CWP: Consider the titration of 150.0 mL of 0.100 M HI by 0.250 M NaOH. a. Calculate the pH after 20.0 mL... Problem 105CWP: Consider the titration of 100.0 mL of 0.100 M HCN by 0.100 M KOH at 25C. (Ka for HCN = 6.2 1010.)... Problem 106CWP: Consider the titration of 100.0 mL of 0.200 M HONH2 by 0.100 M HCI. (Kb for HONH2 = 1.1 108.) a.... Problem 107CWP: Consider the following four titrations (iiv): i. 150 mL of 0.2 M NH3 (Kb = 1.8 105) by 0.2 M HCl... Problem 108CP: Another way to treat data from a pH titration is to graph the absolute value of the change in pH per... Problem 109CP: A buffer is made using 45.0 mL of 0.750 M HC3H5O2 (Ka = 1.3 105) and 55.0 mL of 0.700 M NaC3H5O2.... Problem 110CP: A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where... Problem 111CP: What volume of 0.0100 M NaOH must be added to 1.00 L of 0.0500 M HOCl to achieve a pH of 8.00? Problem 112CP: Consider a solution formed by mixing 50.0 mL of 0.100 M H2SO4, 30.0 mL of 0.100 M HOCI, 25.0 mL of... Problem 113CP: When a diprotic acid. H2A. is titrated with NaOH, the protons on the diprotic acid are generally... Problem 114CP Problem 115CP: The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major... Problem 116CP: Consider the titration curve in Exercise 115 for the titration of Na2Cr3 with HCl. a. If a mixture... Problem 117CP: A few drops of each of the indicators shown in the accompanying table were placed in separate... Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,... Problem 119IP: A buffer solution is prepared by mixing 75.0 mL of 0.275 M fluorobenzoic acid (C7H5O2F) with 55.0 mL... Problem 120IP: A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in... Problem 121IP: Calculate the pH of a solution prepared by mixing 250. mL of 0.174 m aqueous HF (density = 1.10... Problem 122MP: Consider a solution prepared by mixing the foUowing: 50.0 mL of 0.100 M Na3PO4 100.0 mL of 0.0500 M... Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...
Related questions
Polymers are not very soluble in water, but their solubility increases if they have charged groups. (a) Case in, a milk protein,contains many —COO⁻ groups on its side chains. How does the solubility of casein vary with pH? (b) Histones are proteins es-sential to the function of DNA. They are weakly basic due to the presence of side chains with —NH2 and =NH groups. How does the solubility of a histone vary with pH?
Definition Definition Large and very high-molecular-weight substances that consist of hundreds to thousands of repeating units. Polymers are also known as macromolecules. Number-average-molecular weight is the measuring system for the polymers.
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