Problem 1E: Complete the changes in concentrations for each of the following reactions: (a) AgI(s)Ag+(aq)+I(aq)x... Problem 2E: Complete the changes in concentrations for each of the following reactions: (a)... Problem 3E: How do the concentrations of Ag+ and CrO42- in a saturated solution above 1.0 g of solid Ag2CrO4... Problem 4E: How do the concentrations of Pb2+ and S2- change when K2S is added to a saturated solution of PbS? Problem 5E: What additional information do we need to answer the following question: How is the equilibrium of... Problem 6E: Which of the following slightly soluble compounds has a solubility greater than that calculated from... Problem 7E: Which of the following slightly soluble compounds has a solubility greater than that calculated from... Problem 8E: Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the... Problem 9E: Write the ionic equation for the dissolution and the Ksp expression for each of the following... Problem 10E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities... Problem 11E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities... Problem 12E: Use solubility products and predict which of the following salts is the most soluble, in terms of... Problem 13E: Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of... Problem 14E: Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of... Problem 15E: Assuming that no equilibria other than dissolution are involved, calculate the concentration of all... Problem 16E: Assuming that no equilibria other than dissolution are involved, calculate the concentration of all... Problem 17E: Assuming that no equilibria other than dissolution are involved, calculate the concentration of all... Problem 18E: Explain why the changes in concentrations of the common ions in Exercise 15.17 can be neglected. Problem 19E: Explain why the Changes in concentrations of the common ions in Exercise 15.18 cannot be neglected. Problem 20E: Calculate the solubility of aluminum hydroxide, Al(OH)3, in a solution buffered at pH 11.00. Problem 21E: Refer to Appendix J for solubility products for calcium salts. Determine which of the calcium salts... Problem 22E: Most barium compounds are very poisonous; however, barium sulfate is often administered internally... Problem 23E: Public Health Service standards for drinking water set a maximum of 250 mg/L (2.620103M) of SO42-... Problem 24E: Perform the following calculations: (a) Calculate [Ag+] in a saturated aqueous solution of AgBr. (b)... Problem 25E: The solubility product of CaSO42H2O is 2.4105. What mass of this salt will dissolve in 1.0 L of... Problem 26E: Assuming that no equilibria other than dissolution are involved, calculate the concentrations of... Problem 27E: Assuming that no equilibria other than dissolution are involved, calculate the concentrations of... Problem 28E: The following concentrations are found in mixtures of ions in equilibrium with slightly soluble... Problem 29E: The following concentrations are found in mixtures of ions in equilibrium with slightly soluble... Problem 30E: Which of the following compounds precipitates from a solution that has the concentrations indicated?... Problem 31E: Which of the following compounds precipitates from a solution that has the concentrations indicated?... Problem 32E: Calculate the concentration of Tl+ when TICl just begins to precipitate from a solution that is... Problem 33E: Calculate the concentration of sulfate ion when BaSO4 just begins to precipitate from a solution... Problem 34E: Calculate the concentration of Sr2+ when SrF2 starts to precipitate from a solution that is 0.0025 M... Problem 35E: Calculate the concentration of PO43- when Ag3PO4 starts to precipitate from a solution that is... Problem 36E: Calculate the concentration of F- required to begin precipitation of CaF2 in a solution that is... Problem 37E: Calculate the concentration] of Ag+ required to begin precipitation of Ag2CO3 in a solution that is... Problem 38E: What [Ag+] is required to reduce [CO32-] to 8.2104M by precipitation of Ag2CO3? Problem 39E: What [F-] is required to reduce [Ca2+] to 1.0104M by precipitation of CaF2? Problem 40E: A volume of 0.800 L of a 2104 -M Ba(NO3)2 solution is added to 0.200 L of 5104M Li2SO4. Does BaSO4... Problem 41E: Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a... Problem 42E: Iron concentrations greater than 5.4106 M in water used for laundry purposes can cause staining.... Problem 43E: A solution is 0.010 M in both Cu2+ and Cd2+. What percentage of Cd2+ remains in the solution when... Problem 44E: A solution is 0.15 M in both Pb2+ and Ag+. If Cl- is added to this solution, what is [Ag+] when... Problem 45E: What reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M... Problem 46E: A solution contains 1.0105 mol of KBr and 0.10 mol of KCl per liter. AgNO3 is gradually added to... Problem 47E: A solution contains 1.0102 mol of Kl and 0.10 mol of KCl per liter. AgNO3 is gradually added to this... Problem 48E: The calcium ions in human blood serum are necessary for coagulation (Figure 15.5). Potassium... Problem 49E: About 50% of urinary calculi (kidney stones) consist of calcium phosphate, Ca3(PO4)2. The normal... Problem 50E: The pH of normal urine is 6.30, and the total phosphate concentration... Problem 51E: Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production... Problem 52E: Hydrogen sulfide is bubbled into a solution that is 0.10 M in both Pb2+ and Fe2+ and 0.30 M in HCl.... Problem 53E: Perform the following calculations involving concentrations of iodate ions: (a) The iodate ion... Problem 54E: Calculate the molar solubility of AgBr in 0.035 M NaBr (KSP=51013). Problem 55E: How many grams of Pb(OH)2 will dissolve in 500 mL of a 0.050-M PbCl2 solution (KSP=1.21015)? Problem 56E: Use the simulation (http://openstaxcollege.org/l/16solublesalts) from the earlier Link to Learning... Problem 57E: How many grams of Milk of Magnesia, Mg(OH)2 (s) (58.3 g/mol), would be soluble in 200 mL of water.... Problem 58E: Two hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is... Problem 59E: Which of the following carbonates will form first? Which of the following will form last? Explain.... Problem 60E: How many grams of Zn(CN)2(s) (117.44 g/mol) would be soluble in 100 mL of H2O? Include the balanced... Problem 61E: Under what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water? Problem 62E: Explain why the addition of NH3 or HNO3 to a saturated solution of Ag2CO3 in contact with solid... Problem 63E: Calculate the cadmium ion concentration, [Cd2+], in a solution prepared by mixing 0.100 L of 0.0100... Problem 64E: Explain why addition of NH3 or HNO3 to a saturated solution of Cu(OH)2 in contact with solid Cu(OH)2... Problem 65E: Sometimes equilibria fur complex ions are described in terms of dissociation constants. Kd . For the... Problem 66E: Using the value of the formation constant for the complex ion Co(NH3)62+ calculate the dissociation... Problem 67E: Using the dissociation constant, Kd=7.81018, calculate the equilibrium concentrations of Cd2+ and... Problem 68E: Using the dissociation constant, Kd=3.41015, calculate the equilibrium concentrations of Zn2+ and... Problem 69E: Using the dissociation constant, Kd=2.21034, calculate the equilibrium concentrations of Co3+ and... Problem 70E: Using the dissociation constant kd=1*10-44 calculate the equilibrium concentrations of Fe3+ and CN-... Problem 71E: Calculate the mass of potassium cyanide ion that must be added to 100 mL of solution to dissolve... Problem 72E: Calculate the minimum concentration of ammonia needed in 1.0 L of solution to dissolve 3.0103 mol of... Problem 73E: A roll of 35-mm black and white photographic film contains about 0.27 g of unexposed AgBr before... Problem 74E: We have seen an introductory definition of an acid: An acid is a compound that reacts with water and... Problem 75E: Write the Lewis structures of the reactants and product of each of the following equations, and... Problem 76E: Write the Lewis structures of the reactants and product of each of the following equations, and... Problem 77E: Using Lewis structures, write balanced equations for the following reactions: (a) HCI(g)+PH3(g) (b)... Problem 78E: Calculate [HgCl42-] in a solution prepared by adding 0.0200 mol of NaCl to 0.250 L of a 0.100-M... Problem 79E: In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The... Problem 80E: What are the concentrations of Ag+, CN-, and Ag(CN)2- in a saturated solution of AgCN? Problem 81E: In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C)... Problem 82E: The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they... Problem 83E: Boric acid, H3303, is not a Bronsted-Lowry acid but a Lewis acid.. (a) Write an equation for its... Problem 84E: A saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte... Problem 85E: Calculate the equilibrium concentration of Ni2+ in a 1.0-M solution [Ni(NH3)6](NO3)2. Problem 86E: Calculate the equilibrium concentration of Zn2+ in a 0.30-M solution of Zn(CN)42-. Problem 87E: Calculate the equilibrium concentration of Cu2+ in a solution initially with 0.050 M Cu2+ and 1.00 M... Problem 88E: Calculate the equilibrium concentration of Zn2+ in a solution initially with 0.150 M Zn2+ and 2.50 M... Problem 89E: Calculate the Fe3+ equilibrium concentration when 0.0888 mole of K3[Fe(CN)6] is added to a solution... Problem 90E: Calculate the CO2+ equilibrium concentration when 0.100 mole of [CO(NH3)6](NO3)2 is added to a... Problem 91E: The equilibrium constant for the reaction Hg2+(aq)+2Cl(aq)HgCl2(aq) is 1.61013, Is HgCl2 a strong... Problem 92E: Calculate the molar solubility of Sn(OH)2 in a buffer solution containing equal concentrations of... Problem 93E: Calculate the molar solubility of Al(OH)3 in a buffer solution with 0.100 M NH3 and 0.400 M NH4+. Problem 94E: What is the molar solubility of CaF2 in a 0.100-M solution of HF? Ka for HF=7.2104. Problem 95E: What is the molar solubility of BaSO4 in a 0.250-M solution of NaHSO4? Ka for HSO4=1.2102. Problem 96E: What is the molar solubility of Tl(OH)3 in a 0.10-M solution of NH3? Problem 97E: What is the molar solubility of Pb(OH)2 in a 0.138-M solution of CH3NH2? Problem 98E: A solution of 0.075 M CoBr2 is saturated with H2S([H2S]=0.10M). What is the minimum pH at which CoS... Problem 99E: A 0.125-M solution of 0.075 Mn(NO3)2 is saturated with H2S([H2S]=0.10M). At what pH does Mns begin... Problem 100E: Calculate the molar solubility of BaF2 in a buffer solution containing 0.20 M HF and 0.20 M NaF. Problem 101E: Calculate the molar solubility of CdCO3 in a buffer solution containing 0.115 M Na2CO3 and 0.120 M... Problem 102E: To a 0.10-M solution of Pb(NO3)2 is added enough HF(g) to make [HF]=0.10M. (a) Does PbF2 precipitate... Problem 103E: Calculate the concentration of Cd2+ resulting from the dissolution of CdCO3 in a solution that is... Problem 104E: Both AgCl and Agl dissolve in NH3.. (a) What mass of AgI dissolves in 1.0 L of 1.0 M NH3?. (b) VNhat... Problem 105E: Calculate the volume of 1.50 M CH3CO2H required to dissolve a precipitate composed of 350 mg each of... Problem 106E: Even though Ca(OH)2 is an inexpensive base, its limited solubility restricts its use. What is the pH... Problem 107E: What mass of NaCN must be added to 1 L of 0.010 M Mg(NO3)2 in order to produce the first trace of... Problem 108E: Magnesium hydroxide and magnesium citrate function as mild laxatives when they reach the small... Problem 109E: The following question is taken from a Chemistry Advanced Placement Examination and is used with the... Problem 110E: Which of the following compounds, when dissolved in a 0.01-M solution of HClO4, has a solubility... Problem 111E: Which of the following compounds, when dissolved in a 0.01-M solution of HClO4, has a solubility... Problem 112E: What is the effect on the amount of solid Mg(OH)2 that dissolves and the concentrations of Mg2+ and... Problem 113E: What is the effect on the amount of CaHPO4 that dissolves and the concentrations of Ca2+ and HPO4-... Problem 114E: Identify all chemical species present in an aqueous solution of Ca3(PO4)2 and list these species in... Problem 115E: A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of... format_list_bulleted
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Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning