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Problem 79
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 81
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 82
- Referring to Table 17.1, pick an indicator for use in the titration of each acid with a strong base. a. HF
Problem 83
Problem 84
Referring to Table 17.1, pick an indicator for use in the titration of each base with a strong acid. a. CH3NH2
Problem 85a
Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. a. BaSO4
Problem 85b
Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. b. PbBr2
Problem 85c
Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. c. Ag2CrO4
Problem 86
Write balanced equations and expressions for Ksp for the dissolution of each ionic compound. a. CaCO3 b. PbCl2 c. AgI
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 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 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
- 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 97a
Calculate the molar solubility of calcium hydroxide in a solution buffered at each pH. a. pH = 4
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