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Problem 87a
Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. a. AgBr
Problem 87b,c
Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. b. Mg(OH)2 c. CaF2
Problem 88
Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. a. MX (Ksp = 1.27⨉10-36) b. Ag2CrO4 c. Ca(OH)2
Problem 89a
Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27⨉10-11 M
Problem 89b,c
Use the given molar solubilities in pure water to calculate Ksp for each compound. b. PbF2; molar solubility = 5.63⨉10-3 M c. MgF2; molar solubility = 2.65⨉10-4 M
Problem 90a
Use the given molar solubilities in pure water to calculate Ksp for each compound. a. BaCrO4; molar solubility = 1.08⨉10-5 M
Problem 90b,c
Use the given molar solubilities in pure water to calculate Ksp for each compound. b. Ag2SO3; molar solubility = 1.55⨉10-5 M c. Pd(SCN)2; molar solubility = 2.22⨉10-8 M
Problem 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?
Problem 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
- 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.
Problem 93
Problem 94
The solubility of copper(I) chloride is 3.91 mg per 100.0 mL of solution. Calculate Ksp for CuCl.
Problem 95a
Calculate the molar solubility of barium fluoride in each liquid or solution. a. pure water
Problem 95b
Calculate the molar solubility of barium fluoride in each liquid or solution. b. 0.10 M Ba(NO3)2
Problem 95c
Calculate the molar solubility of barium fluoride in each liquid or solution. c. 0.15 M NaF
- Calculate the molar solubility of MX (Ksp = 1.27 × 10^-36) in pure water.
Problem 96a
Problem 96b
Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. b. 0.25 M MCl2
Problem 96c
Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. c. 0.20 M Na2X
Problem 97a
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. a. pH = 4
Problem 97b
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. b. pH = 7
Problem 97c
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. c. pH = 9
Problem 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?
Problem 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
Problem 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
Problem 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.
- 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.
Problem 102
Problem 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.
- 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.
Problem 104
- 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
Problem 105
Problem 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
Problem 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