Ch.17 - Aqueous Ionic Equilibrium

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Ch.17 - Aqueous Ionic Equilibrium

Problema 89b,c

Use the given molar solubilities in pure water to calculate K_sp for each compound. b. PbF₂; molar solubility = 5.63⨉10^-3 M c. MgF₂; molar solubility = 2.65⨉10^-4 M

Problema 90a

Use the given molar solubilities in pure water to calculate K_sp for each compound. a. BaCrO₄; molar solubility = 1.08⨉10^-5 M

Problema 90b,c

Use the given molar solubilities in pure water to calculate K_sp for each compound. b. Ag₂SO₃; molar solubility = 1.55⨉10^-5 M c. Pd(SCN)₂; molar solubility = 2.22⨉10^-8 M

Problema 91

Two compounds with general formulas AX and AX₂ have Ksp = 1.5⨉10^-5. Which of the two compounds has the higher molar solubility?

Problema 92

Consider the compounds with the generic formulas listed and their corresponding molar solubilities in pure water. Which compound has the smallest value of Ksp? a. AX; molar solubility = 1.35⨉10^-4 M b. AX₂; molar solubility = 2.25⨉10^-4 M c. A₂X; molar solubility = 1.75⨉10^-4 M

Problema 93

Refer to the Ksp value from Table 17.2 to calculate the solubility of iron(II) hydroxide in pure water in grams per 100 mL of solution.

Problema 94

The solubility of copper(I) chloride is 3.91 mg per 100.0 mL of solution. Calculate Ksp for CuCl.

Problema 95a

Calculate the molar solubility of barium fluoride in each liquid or solution. a. pure water

Problema 95b

Calculate the molar solubility of barium fluoride in each liquid or solution. b. 0.10 M Ba(NO₃)₂

Problema 95c

Calculate the molar solubility of barium fluoride in each liquid or solution. c. 0.15 M NaF

Problema 96a

Calculate the molar solubility of MX (Ksp = 1.27 × 10^-36) in pure water.

Problema 96b

Calculate the molar solubility of MX (K_sp = 1.27⨉10^-36) in each liquid or solution. b. 0.25 M MCl₂

Problema 96c

Calculate the molar solubility of MX (K_sp = 1.27⨉10^-36) in each liquid or solution. c. 0.20 M Na₂X

Problema 97a

Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. a. pH = 4

Problema 97b

Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. b. pH = 7

Problema 97c

Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. c. pH = 9

Problema 98

Calculate the solubility (in grams per 1.00⨉10² mL of solution) of magnesium hydroxide in a solution buffered at pH = 10. How does this compare to the solubility of Mg(OH)₂ in pure water?

Problema 99

Determine if each compound is more soluble in acidic solution than it is in pure water. Explain. a. BaCO₃ b. CuS c. AgCl d. PbI₂

Problema 100

Determine if each compound is more soluble in acidic solution than it is in pure water. Explain. a. Hg₂Br₂ b. Mg(OH)₂ c. CaCO₃ d. AgI

Problema 101

A solution containing sodium fluoride is mixed with one containing calcium nitrate to form a solution that is 0.015 M in NaF and 0.010 M in Ca(NO₃)₂. Does a precipitate form in the mixed solution? If so, identify the precipitate.

Problema 102

A solution containing potassium bromide is mixed with one containing lead acetate to form a solution that is 0.013 M in KBr and 0.0035 M in Pb(C2H3O2)2. Does a precipitate form in the mixed solution? If so, identify the precipitate.

Problema 103

Predict whether a precipitate will form if you mix 75.0 mL of a NaOH solution with pOH = 2.58 with 125.0 mL of a 0.018 M MgCl₂ solution. Identify the precipitate, if any.

Problema 104

Predict whether a precipitate will form if you mix 175.0 mL of a 0.0055 M KCl solution with 145.0 mL of a 0.0015 M AgNO3 solution, and identify the precipitate, if any.

Problema 105

What is the minimum concentration of KOH required for precipitation to begin for each of the following cation solutions? a. 0.015 M CaCl2 b. 0.0025 M Fe(NO3)2 c. 0.0018 M MgBr2

Problema 106a

Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. a. 0.035 M Ba(NO₃)₂; NaF

Problema 106b

Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. b. 0.085 M CaI₂; K₂SO₄

Problema 106c

Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. c. 0.0018 M AgNO₃; RbCl

Problema 107a

A solution is 0.010 M in Ba²⁺ and 0.020 M in Ca²⁺. a. If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? What minimum concentration of Na₂SO₄ will trigger the precipitation of the cation that precipitates first?

Problema 107b

A solution is 0.010 M in Ba²⁺ and 0.020 M in Ca²⁺. b. What is the remaining concentration of the cation that precipitates first, when the other cation begins to precipitate?

Problema 108

A solution is 0.022 M in Fe2+ and 0.014 M in Mg2+. a. If potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? What minimum concentration of K2CO3 will trigger the precipitation of the cation that precipitates first? b. What is the remaining concentration of the cation that precipitates first when the other cation begins to precipitate?