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Problem 82
Consider the titration curves (labeled a and b) for two weak bases, both titrated with 0.100 M HCl. (a)
(b)
(ii) Which base has the larger Kb?
Problem 83
A 0.229-g sample of an unknown monoprotic acid is titrated with 0.112 M NaOH. The resulting titration curve is shown here. Determine the molar mass and pKa of the acid.
- Is a 0.446-g sample of an unknown monoprotic acid titrated with 0.105 M KOH resulting in a titration curve sufficient to determine the molar mass and pKa of the acid?
Problem 84
Problem 85
A 20.0-mL sample of 0.115 M sulfurous acid (H2SO3) solution is titrated with 0.1014 M KOH. At what added volume of base solution does each equivalence point occur?
Problem 87
Methyl red has a pKa of 5.0 and is red in its acid form and yellow in its basic form. If several drops of this indicator are placed in a 25.0-mL sample of 0.100 M HCl, what color will the solution appear? If 0.100 M NaOH is slowly added to the HCl sample, in what pH range will the indicator change color?
- Phenolphthalein has a pKa of 9.7. It is colorless in its acid form and pink in its basic form. For each of the following pH values, determine whether [In-] > [HIn] and predict the color of a phenolphthalein solution: a. pH = 2.0 b. pH = 5.0 c. pH = 8.0 d. pH = 11.0
Problem 88
Problem 89
Referring to Table 18.1, pick an indicator for use in the titration of each acid with a strong base. a. HF
Problem 90a
Referring to Table 17.1, pick an indicator for use in the titration of each base with a strong acid. a. CH3NH2
Problem 91a
Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. a. BaSO4
Problem 91b
Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. b. PbBr2
Problem 91c
Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. c. Ag2CrO4
Problem 93a
Refer to the Ksp values in Table 18.2 to calculate the molar solubility of each compound in pure water. a. AgBr
Problem 95a
Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27⨉10-11 M
Problem 95b
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 96a
Use the given molar solubilities in pure water to calculate Ksp for each compound. a. BaCrO4; molar solubility = 1.08⨉10-5 M
Problem 96b
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 97
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 98
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
Problem 100
The solubility of copper(I) chloride is 3.91 mg per 100.0 mL of solution. Calculate Ksp for CuCl.
Problem 101a
Calculate the molar solubility of barium fluoride in each liquid or solution. a. pure water
Problem 101b
Calculate the molar solubility of barium fluoride in each liquid or solution. b. 0.10 M Ba(NO3)2
Problem 101c
Calculate the molar solubility of barium fluoride in each liquid or solution. c. 0.15 M NaF
Problem 102b
Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. b. 0.25 M MCl2
Problem 102c
Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. c. 0.20 M Na2X
Problem 103a
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. a. pH = 4
Problem 103b
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. b. pH = 7
Problem 103c
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. c. pH = 9
Problem 104
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 105c
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 107
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.