Brown - Chemistry: The Central Science 14th Edition - Chapter 17

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Ch.17 - Additional Aspects of Aqueous Equilibria

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Brown 14th Edition

Ch.17 - Additional Aspects of Aqueous Equilibria

Problem 58b
Calculate the solubility of LaF₃ in grams per liter in (b) 0.010 M KF solution.
Problem 58c
Calculate the solubility of LaF₃ in grams per liter in (c) 0.050 M LaCl₃ solution.
Problem 59
Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF2(s). Solid CaCl2 is then added to the solution. (b) Will the concentration of Ca2+ ions in solution increase or decrease? (c) Will the concentration of F- ions in solution increase or decrease?
Problem 59a
Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF21s2. Solid CaCl2 is then added to the solution. (a) Will the amount of solid CaF2 at the bottom of the beaker increase, decrease, or remain the same?
Problem 61
Calculate the solubility of Mn(OH)₂ in grams per liter when buffered at pH (a) 7.0 (b) 9.5 (c) 11.8.
Problem 62a
Calculate the molar solubility of Ni(OH)₂ when buffered at pH (a) 8.0.
Problem 62b
Calculate the molar solubility of Ni(OH)₂ when buffered at pH (b) 10.0.
Problem 62c
Calculate the molar solubility of Ni(OH)₂ when buffered at pH (c) 12.0.
Problem 63
Which of the following salts will be substantially more soluble in acidic solution than in pure water: (a) ZnCO3, (b) ZnS, (c) BiI3, (d) AgCN, (e) Ba3(PO4)2?
Problem 64
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a strong acid: (a) MnS (b) PbF₂ (c) AuCl₃ (e) CuBr (d) Hg₂C₂O₄.
Problem 65
From the value of Kf listed in Table 17.1, calculate the concentration of Ni2 +1aq2 and Ni1NH326 2+ that are present at equilibrium after dissolving 1.25 g NiCl2 in 100.0 mL of 0.20 M NH31aq2.
Problem 66
From the value of Kf listed in Table 17.1, calculate the concentration of NH3 required to just dissolve 0.020 mol of NiC2O4 (Ksp = 4 * 10^-102) in 1.00 L of solution? (Hint: You can neglect the hydrolysis of C2O4^2- because the solution will be quite basic.)
Problem 67
Use values of Ksp for AgI and Kf for [Ag(CN)2]- to (a) calculate the molar solubility of AgI in pure water. (b) calculate the equilibrium constant for the reaction AgI(s) + 2 CN⁻(aq) ⇌ [Ag(CN)2]⁻(aq) + I⁻(aq). (c) determine the molar solubility of AgI in a 0.100 M NaCN solution.
Problem 68
Using the value of Ksp for Ag2S, Ka1 and Ka2 for H2S, and Kf = 1.1 * 10^5 for AgCl2^-, calculate the equilibrium constant for the following reaction: Ag2S (s) + 4 Cl^- (aq) + 2 H^+ (aq) ⇌ 2 AgCl2^- (aq) + H2S (aq)
Problem 69
(a) Will Ca(OH)2 precipitate from solution if the pH of a 0.050 M solution of CaCl2 is adjusted to 8.0? (b) Will Ag2SO4 precipitate when 100 mL of 0.050 M AgNO3 is mixed with 10 mL of 5.0 * 10^-2 M Na2SO4 solution?
Problem 71
Calculate the minimum pH needed to precipitate Mn1OH22 so completely that the concentration of Mn2 +1aq2 is less than 1 mg per liter [1 part per billion (ppb)].
Problem 72
Suppose that a 10-mL sample of a solution is to be tested for I- ion by addition of 1 drop (0.2 mL) of 0.10 M Pb1NO322. What is the minimum number of grams of I- that must be present for PbI21s2 to form?
Problem 73
A solution contains 2.0 * 10^-4 M Ag^+ (aq) and 1.5 * 10^-3 M Pb^2+ (aq). If NaI is added, will AgI (Ksp = 8.3 * 10^-17) or PbI2 (Ksp = 7.9 * 10^-9) precipitate first? Specify the concentration of I^- (aq) needed to begin precipitation.
Problem 74a
A solution of Na₂SO₄ is added dropwise to a solution that is 0.010 M in Ba²⁺(aq) and 0.010 M in Sr²⁺(aq). (a) What concentration of SO₄^2- is necessary to begin precipitation? (Neglect volume changes. BaSO₄: Ksp = 1.1⨉10^-10; SrSO₄: Ksp = 3.2⨉10^-7.)
Problem 74b
A solution of Na₂SO₄ is added dropwise to a solution that is 0.010 M in Ba²⁺(aq) and 0.010 M in Sr²⁺(aq). (b) Which cation precipitates first?
Problem 74c
A solution of Na₂SO₄ is added dropwise to a solution that is 0.010 M in Ba²⁺(aq) and 0.010 M in Sr²⁺(aq). (c) What is the concentration of SO₄^2-(aq) when the second cation begins to precipitate?
Problem 75
A solution contains three anions with the following concentrations: 0.20 M CrO4^2-, 0.10 M CO3^2-, and 0.010 M Cl-. If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Ag2CrO4 (Ksp = 1.2 * 10^-12), Ag2CO3 (Ksp = 8.1 * 10^-12), or AgCl (Ksp = 1.8 * 10^-10)?
Problem 76
A 1.0 M Na2SO4 solution is slowly added to 10.0 mL of a solution that is 0.20 M in Ca2+ and 0.30 M in Ag+. (a) Which compound will precipitate first: CaSO4 (Ksp = 2.4 * 10^-5) or Ag2SO4 (Ksp = 1.5 * 10^-5)?
Problem 77
A solution containing several metal ions is treated with dilute HCl; no precipitate forms. The pH is adjusted to about 1, and H₂S is bubbled through. Again, no precipitate forms. The pH of the solution is then adjusted to about 8. Again, H₂S is bubbled through. This time a precipitate forms. The filtrate from this solution is treated with (NH₄)₂HPO₄. No precipitate forms. Which of these metal cations are either possibly present or definitely absent: Al³⁺, Na⁺, Ag⁺, Mg²⁺?
Problem 79a,b
In the course of various qualitative analysis procedures, the following mixtures are encountered: (a) Zn²⁺ and Cd²⁺. (b) Cr(OH)₃ and Fe(OH)₃ Suggest how each mixture might be separated.
Problem 79c,d
In the course of various qualitative analysis procedures, the following mixtures are encountered: (c) Mg²⁺ and K⁺ (d) Ag⁺ and Mn²⁺. Suggest how each mixture might be separated.
Problem 80c
Suggest how the cations in each of the following solution mixtures can be separated: (c) Pb2 + and Al3 +.
Problem 81b
(b) What is the most significant difference between the sulfides precipitated in group 2 and those precipitated in group 3?
Problem 83
Derive an equation similar to the Henderson–Hasselbalch equation relating the pOH of a buffer to the pKb of its base component.
Problem 84
Rainwater is acidic because CO21g2 dissolves in the water, creating carbonic acid, H2CO3. If the rainwater is too acidic, it will react with limestone and seashells (which are principally made of calcium carbonate, CaCO3). Calculate the concentrations of carbonic acid, bicarbonate ion 1HCO3-2 and carbonate ion 1CO32 - 2 that are in a raindrop that has a pH of 5.60, assuming that the sum of all three species in the raindrop is 1.0 * 10-5 M.