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문제 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
문제 90a
Use the given molar solubilities in pure water to calculate Ksp for each compound. a. BaCrO4; molar solubility = 1.08⨉10-5 M
문제 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
문제 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?
문제 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.
문제 93
문제 94
The solubility of copper(I) chloride is 3.91 mg per 100.0 mL of solution. Calculate Ksp for CuCl.
문제 95a
Calculate the molar solubility of barium fluoride in each liquid or solution. a. pure water
문제 95b
Calculate the molar solubility of barium fluoride in each liquid or solution. b. 0.10 M Ba(NO3)2
문제 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.
문제 96a
문제 96b
Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. b. 0.25 M MCl2
문제 96c
Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. c. 0.20 M Na2X
문제 97a
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. a. pH = 4
문제 97b
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. b. pH = 7
문제 97c
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. c. pH = 9
문제 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?
문제 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
문제 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
문제 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.
문제 102
문제 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.
문제 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
문제 105
문제 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
문제 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
문제 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
문제 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?
문제 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?
- 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?
문제 108