Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
79. Calculate the molar solubility of BaCO3 in a 0.10 M solution of Na2CO3(aq). (Ksp
(BaCO3) = 8.1 x 10-9)
80. Calculate the molar solubility of CaF2 in a 0.25 M solution of NaF(aq). (Ksp (CaF2) = 4.0
x 10–11)
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
81. Calculate the molar solubility of AgCl in a 0.15 M solution of NH3(aq).
(Ksp (AgCl) = 1.6 x 10–10; Kf (Ag(NH3)2+) = 1.5 x 107)
82. Calculate the molar solubility of AgBr in a 0.25M solution of NH3(aq) (Ksp (AgBr) = 7.7
x 10–13 ; Kf (Ag(NH3)2+) = 1.5 x 107.
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
83. Calculate the molar solubility of Fe(OH)2 in a solution with pH = 13.15.
(Ksp Fe(OH)2 = 1.6 x 10–14)
84. Calculate the molar solubility of Mg(OH)2 in a solution with pH = 12.20.
(Ksp (Mg(OH)2 = 1.2 x 10–11)
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
85. Find the concentration of Pb2+ ions in a solution made by adding 5.00 g of lead(II) iodide
to 500. mL of 0.150 M KI. [For PbI2, Ksp = 1.39 10–8.]
86. Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium
fluoride to 750. mL of 0.125 M NaF. [For CaF2, Ksp = 3.95 10–11.]
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
87. A saturated sodium carbonate solution at 0C contains 7.1 g of dissolved sodium
carbonate per 100. mL of solution. The solubility product constant for sodium carbonate at
this temperature is
88. A saturated sodium carbonate solution at 100C contains 45.5 g of dissolved sodium
carbonate per 100. mL of solution. The solubility product constant for sodium carbonate at
this temperature is
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
89. Which of the following compounds is more soluble in acidic solution than in pure neutral
water?
90. Which of the following compounds is more soluble in acidic solution than in pure neutral
water?
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
91. Which of the following compounds is more soluble in a 0.10 M NH3(aq) solution than in
pure neutral water?
92. Which of the following compounds is more soluble in a 0.10 M NaCN solution than in
pure neutral water?
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
93. What volume of 0.0500 M sodium hydroxide should be added to 250. mL of 0.100 M
HCOOH to obtain a solution with a pH of 4.50? [Ka(HCOOH) = 1.7 10–4]
94. What volume of 0.200 M potassium hydroxide should be added to 300. mL of 0.150 M
propanoic acid (C2H5COOH) to obtain a solution with a pH of 5.25? [Ka(C2H5COOH) = 1.34
10–5]
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
95. Calculate the pH of a solution that is 0.15 M CH3COOH and 0.75 M CH3COONa.
96. Calculate the pH of a solution that is 0.20M NH3(aq) and 0.35 M NH4Cl(aq).
(Kb(NH3) = 1.8 x 10-5)
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
97. 500. mL of a solution containing 1.5 M NH3(aq) is mixed with 500. mL of a solution
containing 0.50M of HCl(aq). What is the pH of the final solution?
(Kb(NH3) = 1.8 x 10-5)
98. 500. mL of a solution containing 1.5 M NH4Cl(aq) is mixed with 500. mL of a solution
containing 0.50M of NaOH(aq). What is the pH of the final solution?
(Kb(NH3) = 1.8 x 10-5)
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
99. What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, Ka =
1.7 10–4.)
100.
Select True or False: The equation shown here is the net reaction that occurs when a strong acid is added to a CO32–/HCO3–
buffer solution (for carbonic acid, Ka1 = 4.2 10–7, Ka2 = 2.4 10–8): CO32– + H+ → HCO3– and HCO3– + H+ → H2CO3
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
101.
Select True or False: The equation shown here is the net reaction that occurs when a strong base is added to a CO32–/HCO3–
buffer solution (for carbonic acid, Ka1 = 4.2 10–7, Ka2 = 2.4 10–8): HCO3– + OH– → CO32– + H2O
102. Calculate the percent ionization of formic acid in a 0.010 M HCOOH solution.
(Ka = 1.7 10–4)
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
103. Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and
0.005 M HCOONa. (Ka = 1.7 10–4)
104. Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and
0.050 M HCOONa. (Ka = 1.7 10–4)
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
105. What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer
with a pH of 5.20? [Ka(C6H5COOH) = 6.5 10–5]
106.
Select True or False: The net ionic equation for the reaction that occurs when a small amount of hydrochloric acid is added to
a buffer solution containing NH4Cl and NH3 is correctly shown here: H+ + H2O + NH3 → NH4+
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
107.
Select True or False: The net ionic equation for the reaction occurring when a small amount of sodium hydroxide solution is
added to a buffer solution containing NH4Cl and NH3 is correctly shown here: NaOH + NH4+ → NH3 + H2O + Na+
108.
Select True or False: The net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a
NaNO2/HNO2 buffer is correctly shown here: H+ + NO2– → HNO2
109.
Select True or False: The net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to
a NaNO2/HNO2 buffer is correctly shown here:
OH– + HNO2 → NO2– + H2O
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
110. 550. mL of a 0.40M solution of NaOH is titrated with 0.25 M HCl. Calculate the pH of
the solution after 650. mL of the HCl has been added.
111. 550. mL of a 0.40M solution of NaOH is titrated with 0.25 M HCl. Calculate the pH of
the solution after 1.10 L of HCl has been added.
Chapter 16 – Acid-Base Equilibria and Solubility Equilibria
112. Calculate the pH at the equivalence point for the titration of 0.25 M CH3COOH with
0.25 M NaOH. (For CH3COOH, Ka= 1.8 10–5.)
113. Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M
NaOH. (Ka = 4.9 10–10 for HCN)