Ch.20

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Solid silver nitrate is added slowly to a solution that is 0.0010 M in sodium chloride and 0.0010 M in sodium bromide. What % of the bromide ions remain in solution, i.e., unprecipitated, just before silver chloride begins to precipitate? Ksp for AgCl = 1.8 × 10−10, Ksp for AgBr = 3.3 × 10−13 a. 0.18% b. 0.018% c. 0.0010% d. 0.00010% e. 0.0018%

a. 0.18%

The solubility product constant for MgF2 is 6.4 × 10−9. How many grams of MgF2 will dissolve in 150 mL of H2O at 25°C? a. 1.1 × 10^−2 g b. 5.8 × 10^−3 g c. 4.7 × 10^−1 g d. 6.0 × 10^−4 g e. 2.2 × 10^−3 g

a. 1.1 × 10^−2 g

Calculate the molar solubility of AgCl at 25°C. Ksp = 1.8 × 10−10. a. 1.3 × 10^−5 M b. 1.7 × 10^−5 M c. 4.2 × 10^−5 M d. 4.6 × 10^−5 M e. 1.8 × 10^−10 M

a. 1.3 × 10^−5 M

Calculate the molar solubility of nickel phosphate at 25°C. Its Ksp is 5.0 × 10^−31. a. 3.4 × 10^−7 M b. 8.7 × 10^−7 M c. 6.1 × 10^−7 M d. 7.1 × 10^−16 M e. 5.0 × 10^−11 M

a. 3.4 × 10^−7 M

Calculate the [Zn2+] in a solution which is initially 0.30 M in [Zn(CN)4]2− ions at 25°C. Kd for [Zn(CN)4]2− = 1 × 10−19. a. 4 × 10^−5 M b. 6 × 10^−8 M c. 5 × 10^−6 M d. 1 × 10^−3 M e. 3 × 10^−4 M

a. 4 × 10^−5 M

At 25°C the Ksp for MgCO3 is 4.0 × 10−5 and that for BaCO3 is 8.1 × 10−9. Assuming both magnesium ions and barium ions are present in 1.0 × 10−3 M concentrations, what is the equilibrium concentration of carbonate ions that will precipitate the maximum concentration of Ba2+ without precipitating any Mg2+ at 25°C? a. 4.0 × 10^−2 M b. 4.2 × 10^−3 M c. 3.5 × 10^−3 M d. 5.8 × 10^−2 M e. 3.2 × 10^−2 M

a. 4.0 × 10^−2 M

The molar solubility of manganese(II) hydroxide, Mn(OH)2, is 2.26 x 10-5 M. The solubility product constant, Ksp, for manganese(II) hydroxide is: a. 4.6 x 10^-14 b. 2.3 x 10^-14 c. 5.1 x 10^-10 d. 2.0 x 10^-9 e. 4.5 x 10^-11

a. 4.6 x 10^-14

The hydroxide ion concentration of a saturated solution of Cu(OH)2 is M. What is the solubility product constant for Cu(OH)2? a. 4.80 x 10^-20 b. 3.84 x 10^-19 c. 9.60 x 10^-20 d. 6.77 x 10^-4 e. 7.71 x 10^-3

a. 4.80 x 10^-20

What is the molar solubility of AgCl in 0.10 M NH3 at 25°C? Ksp is 1.8 × 10−10 for AgCl and Kd for [Ag(NH3)2+] is 5.9 × 10−8. a. 4.98 × 10^3 M b. 3.06 × 10^−3 M c. 9.44 × 10^−4 d. 5.53 × 10^−3 M e. 1.34 × 10^−5 M

a. 4.98 × 10^3 M

The molar solubility for copper(II) sulfide in water is 8.53 x 10-19M. What is the Ksp? a. 7.28 x 10^-37 b. 2.48 x 10^-54 c. 6.21 x 10^-55 d. 1.63 x 10^-89 e. 4.52 x 10^-91

a. 7.28 x 10^-37

Calculate the solubility of Mg(OH)2 in g per 100. mL of water. Ksp = 1.5 × 10−11. a. 9.1 × 10^−4 g/100. mL b. 3.6 × 10^−3 g/100. mL c. 6.6 × 10^−5 g/100. mL d. 1.8 × 10^−3 g/100. mL e. 5.0 × 10^−6 g/100. mL

a. 9.1 × 10^−4 g/100. mL

The concentration of strontium carbonate in a saturated aqueous solution at 25°C is M. What is the Ksp of this sparingly soluble salt? a. 9.30 x 10^-10 b. 1.13 x 10^-13 c. 2.34 x 10^-17 d. 5.52 x 10^-3 e. 3.12 x 10^-2

a. 9.30 x 10^-10

The solubility of strontium carbonate in water at 25°C is g/L. What is the Ksp of this sparingly soluble salt? a. 9.30 x 10^-10 b. 1.13 x 10^-13 c. 2.34 x 10^-17 d. 5.52 x 10^-3 e. 3.12 x 10^-2

a. 9.30 x 10^-10

The Ksp for Zn3(AsO4)2 is 1.1 × 10−27. When 100 mL of 5.5 × 10−4 M Zn2+ is mixed with 50 mL of 1.2 × 10−4 M AsO43−, which of the following statements is true? a. A precipitate forms, because Qsp > Ksp. b. A precipitate forms, because Qsp < Ksp. c. No precipitate forms, because Qsp > Ksp. d. No precipitate forms, because Qsp < Ksp. e. None of these statements is true.

a. A precipitate forms, because Qsp > Ksp.

A solution contains 0.05 M Au+, 0.05 M Cu+, and 0.05 M Ag+ ions. When solid NaCl is added to the solution, what is the order in which the chloride salts will begin to precipitate? Ksp(AgCl) = 1.8 × 10−10, Ksp(AuCl) = 2.0 × 10−13, Ksp(CuCl) = 1.9 × 10−7 a. AuCl > AgCl > CuCl b. AuCl > AgCl > NaCl c. AgCl > CuCl > AuCl d. CuCl > AgCl > AuCl e. NaCl > CuCl > AgCl

a. AuCl > AgCl > CuCl

Which of the following solubility product expressions is incorrect? a. Cu2S, Ksp = [Cu+][S2−] b. Co2S3, Ksp = [Co3+]2[S2−]3 c. Ni(CN)2, Ksp = [Ni2+][CN−]2 d. AuI, Ksp = [Au+][I−] e. Cr(OH)3, Ksp = [Cr3+][OH−]3

a. Cu2S, Ksp = [Cu+][S2−]

When 12.0 mL of a 7.13 x 10-4 M manganese(II) iodide, MnI2, solution is combined with 22.0 mL of 5.17 x 10-4 M potassium hydroxide, does a precipitate form? (Ksp for manganese(II) hydroxide is 4.6 x 10-14) a. Mn(OH)2 will precipitate until the solution is saturated b. The solution is unsaturated - no precipitate forms c. The concentration of iodide ions is reduced by the addition of OH- ions d. One must know Ksp for MnI2 to make a prediction e. The presence of KOH will raise the solubility of MnI2

a. Mn(OH)2 will precipitate until the solution is saturated

The solubility product constant, Ksp, for ZnCO3 is 1.5 x 10-11 at 25oC and it is 3.47 x 10-11 at 45oC. Is the dissolution of ZnCO3 an endothermic or exothermic process? a. endothermic b. exothermic c. not enough information to tell.

a. endothermic

The solubility of magnesium carbonate, MgCO3, can be increased by acidifying the solution in which MgCO3 is suspended. This is an example of dissolution via ____. a. formation of a weak electrolyte b. reduction of the anion c. oxidation of the anion d. formation of a complex ion e. changing an ion to another species which is not a weak electrolyte

a. formation of a weak electrolyte

When we mix together, from separate sources, the ions of a slightly soluble ionic salt, the salt will begin to precipitate if Qsp ____ Ksp, and will continue to precipitate until Qsp ____ Ksp. a. is greater than; equals b. is less than; is greater than c. is less than; equals d. equals; is less than e. equals; is greater than

a. is greater than; equals

What mass of Zn(OH)2 is contained in 1.0 liter of saturated solution? Ksp = 4.5 × 10−17. a. 0.00011 g b. 0.00022 g c. 0.00044 g d. 0.010 g e. 0.016 g

b. 0.00022 g

Calculate the number of moles of ammonia needed to dissolve 0.0010 mole of silver chloride in 4000. mL of solution at 25°C. Ksp for AgCl is 1.8 × 10−10 and the dissociation constant for [Ag(NH3)2]+ is 6.3 × 10−8. a. 0.16 mole b. 0.021 mole c. 14 moles d. 0.28 mole e. 1.5 moles

b. 0.021 mole

AgCl would be least soluble at 25°C in ____. a. pure water b. 0.1 M CaCl2 c. 0.1 M HCl d. 0.1 M HNO3 e. It is equally soluble in all of these substances.

b. 0.1 M CaCl2

A 2.0-liter volume of a solution is 4.2 × 10−5 M in Mn(NO3)2 and 0.10 M in ammonia. How many moles of NH4NO3 are required to prevent the precipitation of Mn(OH)2? Ksp for Mn(OH)2 = 4.6 × 10−14 and Kb for NH3 = 1.8 × 10−5. a. 0.62 mol b. 0.11 mol c. 0.048 mol d. 0.24 mol e. 0.033 mol

b. 0.11 mol

What minimum concentration of ammonium ion (from ammonium chloride) is necessary to prevent the precipitation of Mn(OH)2 from a solution which is to be made 0.030 M in Mn(NO3)2 and 0.030 M in aqueous ammonia? The solubility product for Mn(OH)2 is 4.6 × 10−14, and the ionization constant for aqueous ammonia is 1.8 × 10−5. a. 0.18 M b. 0.44 M c. 0.54 M d. 0.72 M e. 0.88 M

b. 0.44 M

The molar solubility of lead(II) chloride (PbCl2) is 1.6 x 10-2 M. What is the solubility product constant, Ksp, of PbCl2? a. 4.9 x 10^-2 b. 1.7 x 10^-5 c. 8.5 x 10^-6 d. 4.2 x 10^-6 e. 6.9 x 10^-6

b. 1.7 x 10^-5

Calculate the concentration of carbonate ion in a saturated solution of calcium carbonate to which calcium chloride has been added until [Ca2+] = 0.015 M at 25°C. Ksp for CaCO3 = 2.8 × 10−9. a. 4.2 × 10^−11 M b. 1.9 × 10^−7 M c. 1.2 × 10^−5 M d. 6.3 × 10^−13 M e. 1.5 × 10^−2 M

b. 1.9 × 10^−7 M

The solubility of Ce(OH)3 is 9.9 × 10−4 g per liter at 25°C. Calculate the solubility product for Ce(OH)3. a. 5.2 × 10^−6 b. 2.0 × 10^−20 c. 7.3 × 10^−20 d. 4.0 × 10^−14 e. 1.6 × 10^−18

b. 2.0 × 10^−20

Calculate [Al3+] in a saturated Al(OH)3 solution at 25°C. Ksp = 1.9 × 10−33 a. 6.6 × 10^−9 M b. 2.9 × 10^−9 M c. 1.5 × 10^−17 M d. 8.4 × 10^−18 M e. 1.5 × 10^−7 M

b. 2.9 × 10^−9 M

The solubility of cerium periodate, Ce(IO4)4, is 0.015 g/mL of water at 25°C. Calculate its solubility product constant. Its formula weight is 904 g/mol. a. 8.1 × 10^−14 b. 3.2 × 10^−7 c. 9.4 × 10^−24 d. 4.1 × 10^−12 e. 6.9 × 10^−22

b. 3.2 × 10^−7

A student measures the molar solubility of iron(II) carbonate, FeCO3, in a water solution to be 6.06 x 10-6 M. Based on her data, the solubility product constant for this compound is: a. 1.21 x 10^-5 b. 3.67 x 10^-11 c. 8.90 x 10^-27 d. 8.17 x 10^-27 e. 1.06 x 10^-25

b. 3.67 x 10^-11

Calculate the concentration of F− ions in saturated CaF2 solution at 25°C. Ksp = 3.9 × 10−11. a. 2.1 × 10^−4 M b. 4.3 × 10^−4 M c. 0.016 M d. 0.032 M e. 0.10 M

b. 4.3 × 10^−4 M

Ksp for silver arsenate is 1.1 × 10−20. What is the molar solubility of Ag3AsO4? a. 2.2 × 10^−7 M b. 4.5 × 10^−6 M c. 6.2 × 10^−8 M d. 4.1 × 10^−7 M e. 1.0 × 10^−10 M

b. 4.5 × 10^−6 M

Calculate the concentration of Cu2+ ions in a 0.010 M [Cu(NH3)4]2+ solution at 25°C. Kd for [Cu(NH3)4]2+ = 8.5 × 10−13 a. 1.3 × 10^−3 M b. 5.1 × 10^−4 M c. 6.3 × 10^−5 M d. 8.7 × 10^5 M e. 1.3 × 10^−6 M

b. 5.1 × 10^−4 M

How many grams of Mn(OH)3 will dissolve in 1350 mL of water at 25°C? Ksp = 1.0 × 10−36 a. 4.6 × 10^−8 g b. 6.3 × 10^−8 g c. 5.9 × 10^−10 g d. 1.4 × 10^−7 g e. 9.3 × 10^−7 g

b. 6.3 × 10^−8 g

It is found that the concentration of Pb2+ in a saturated solution of lead(II) bromide is 1.2 × 10-2 M. What is Ksp for PbBr2? a. 1.7 × 10^-6 b. 6.6 × 10^-6 c. 1.4 × 10^-4 d. 3.5 × 10^-2 e. 3.1 × 10^-7

b. 6.6 × 10^-6

What concentration of Al3+ must be exceeded in a solution buffered at pH = 4.80 in order to initiate precipitation of Al(OH)3 at 25°C? Ksp for Al(OH)3 = 1.9 × 10−33. a. 6.3 × 10^−10 M b. 7.6 × 10^−6 M c. 4.1 × 10^−4 M d. 5.3 × 10^−7 M e. 2.2 × 10^−8 M

b. 7.6 × 10^−6 M

The molar solubility of BaCO3 is 9.0 × 10−5 M at 25°C. What is the solubility product constant for BaCO3? a. 1.2 × 10^−8 b. 8.1 × 10^−9 c. 5.3 × 10^−12 d. 4.0 × 10^−15 e. 6.7 × 10^−11

b. 8.1 × 10^−9

Calculate the pH of a saturated aqueous solution of Co(OH)2. Ksp is 2.5 × 10−16. a. 8.60 b. 8.90 c. 9.10 d. 9.20 e. 9.40

b. 8.90

A solution contains 0.10 M Ca2+ and 0.10 M Mg2+. What pH range would result in only Mg(OH)2 precipitating? Ksp for Ca(OH)2 is 6.5 × 10−6 and for Mg(OH)2 is 7.1 × 10−12. a. 3.85 < pH < 9.82 b. 8.92 < pH < 11.91 c. 2.85 < pH < 8.81 d. 9.00 < pH < 13.00 e. 8.62 < pH < 11.61

b. 8.92 < pH < 11.91

A solution is 1.0 × 10−3 M in Mg(NO3)2 and 1.0 × 10−3 M in Cd(NO3)2. Some solid NaOH is added slowly. What percentage of the Cd2+ originally in solution has precipitated as Cd(OH)2 at the point at which Mg(OH)2 just begins to precipitate? Ksp for Cd(OH)2 is 1.2 × 10−14 and Ksp for Mg(OH)2 is 1.5 × 10−11. a. 98.12% b. 99.92% c. 99.63% d. 98.73% e. 99.52%

b. 99.92%

Solid sodium chloride is added to a solution that is 0.0100M in silver nitrate and 0.0100 M in lead(II) nitrate. Assuming no volume change, calculate the percent of silver that will be precipitated when the lead chloride just begins to precipitate. Ksp = 1.8 × 10−10 for AgCl Ksp = 1.7 × 10−5 for PbCl2 a. 99.8941% b. 99.9996% c. 99.9989% d. 95.9000% e. 98.9413%

b. 99.9996%

Given the following values of Ksp for four slightly soluble sulfides at 25°C. Sulfide Ksp Sulfide Ksp CdS 3.6 × 10−29 PbS 8.4 × 10−28 CuS 8.7 × 10−36 MnS 5.1 × 10−15 Which one of the following ions exists in the lowest concentration in a solution in which the sulfide ion concentration had been fixed at some (fairly large) constant value at 25°C? a. Cd2+ b. Cu2+ c. Pb2+ d. Mn2+ e. Cannot be answered without knowing the sulfide ion concentration.

b. Cu2+

If X = the molar solubility (mol/L) of Ni(OH)2, which of the following represents the correct relationship between the Ksp and X, the molar solubility of Ni(OH)2? a. Ksp = 4 X^2 b. Ksp = 4 X^3 c. Ksp = 2 X^2 d. Ksp = X^3 e. Ksp = X^2

b. Ksp = 4 X^3

If a solution of 0.10 M HI is mixed with a solution of 0.10 M Sn(ClO3)2, what possible precipitate may form? a. Sn(ClO3)2 b. SnI2 c. HClO3 d. SnI4 e. None is possible.

b. SnI2

A solution contains 0.025 M Ba2+. If 9.7 g of Na2CO3 is added to 1.0 L of this solution, what percentage of Ba2+ remains in solution? Assume no change in volume occurs. = 8.1 × 10−9. a. 27.3 % b. 6.6 % c. 0.00049 % d. 0.000012 % e. 0.025 %

c. 0.00049 %

If a solution is to be made 0.010 M in Mg(NO3)2 and 0.20 M in aqueous NH3, how many mol/L of NH4Cl are required to prevent the precipitation of Mg(OH)2 at 25°C? The Kb for aqueous NH3 is 1.8 × 10−5 and the Ksp for Mg(OH)2 is 1.5 × 10−11. a. 0.054 b. 0.56 c. 0.092 d. 1.8 e. 0.86

c. 0.092

At 25°C, 1.4 × 10−5 mole of Cd(OH)2 dissolves to give 1.0 liter of saturated aqueous solution. What is the solubility product for Cd(OH)2? a. 1.7 × 10^−5 b. 2.9 × 10^−10 c. 1.1 × 10^−14 d. 5.8 × 10^−15 e. 4.1 × 10^−12

c. 1.1 × 10^−14

Calculate the minimum concentration of NH3 necessary in 1.0 liter of solution to just dissolve 3.0 × 10−3 mole of AgBr at 25°C. Ksp for AgBr = 3.3 × 10−13, Kd for [Ag(NH3)2]+ = 6.3 × 10−8. a. 6.2 M b. 8.6 M c. 1.3 M d. 0.18 M e. 0.067 M

c. 1.3 M

One liter of saturated zinc hydroxide solution contains 0.00022 g of dissolved Zn(OH)2. Calculate Ksp for Zn(OH)2. a. 4.8 × 10^−12 b. 2.6 × 10^−16 c. 4.5 × 10^−17 d. 7.1 × 10^−14 e. 1.1 × 10^−17

c. 4.5 × 10^−17

What concentration of NH3 must be present in 4.0 × 10−3 M Ag+ to prevent the precipitation of AgCl when [Cl−] reaches 1.0 × 10−3 M? Ksp for AgCl = 1.8 × 10−10 and Kd for [Ag(NH3)2]+ = 6.3 × 10−8. a. 7.4 × 10^−4 M b. 6.1 × 10^−3 M c. 4.5 × 10^−2 M d. 1.6 × 10^−2 M e. 8.5 × 10^−1 M

c. 4.5 × 10^−2 M

The Ksp for magnesium arsenate is 2.1 × 10−20 at 25°C. What is the molar solubility of Mg3(AsO4)2 at 25°C? a. 6.7 × 10^−3 M b. 3.6 × 10^−4 M c. 4.5 × 10^−5 M d. 7.0 × 10^−5 M e. 1.4 × 10^−6 M

c. 4.5 × 10^−5 M

How many grams of AgCl will dissolve in 1.0 L of 0.25 M CaCl2? Ksp (AgCl) = 1.8 × 10−10 a. 3.6 × 10^−10 b. 1.0 × 10^−7 c. 5.1 × 10^−8 d. 1.3 × 10^−8 e. 7.2 × 10^−10

c. 5.1 × 10^−8

The value of Ksp for SrSO4 is 2.8 × 10−7. What is the molar solubility of SrSO4? a. 7.6 × 10^−7 M b. 5.8 × 10^−13 M c. 5.3 × 10^−4 M d. 5.7 × 10^−3 M e. 1.3 × 10^−8 M

c. 5.3 × 10^−4 M

Calculate the concentration of cadmium ions in a 0.10 M [Cd(CN)4]2− solution. The complex ion dissociates: [Cd(CN)4]2− Cd2+ + 4CN− and its dissociation constant is 7.8 × 10−18. a. 3.0 × 10^−5 M b. 5.7 × 10^−5 M c. 7.9 × 10^−5 M d. 9.8 × 10^−5 M e. 2.2 × 10^−4 M

c. 7.9 × 10^−5 M

Which of the following salts would be expected to be more soluble in acidic solution than in pure water? a. AgBr b. Hg2I2 c. CaF2 d. PbCl2 e. BaSO4

c. CaF2

What is the solubility product expression for Co(OH)3? a. Ksp = [Co3+][3OH-] b. Ksp = 3[Co3+][OH-]3 c. Ksp = [Co3+][OH-]3 d. Ksp = [Co3+][3OH-]3 e. Ksp = [Co3+][OH-]

c. Ksp = [Co3+][OH-]3

If a solution is 0.10 M in magnesium nitrate and then is also made 0.10 M in aqueous ammonia, what possible precipitate could form? a. Mg(NO3)2 b. NH4NO3 c. Mg(OH)2 d. NH4OH e. No possible precipitate

c. Mg(OH)2

Which of the following has the lowest molar solubility in water at 25°C? a. Ni(CN)2, Ksp = 3.0 × 10−23 b. ZnS, Ksp = 1.1 × 10−21 c. PbS, Ksp = 8.4 × 10−28 d. Co3(AsO4)2, Ksp = 7.6 × 10−29 e. CaF2, Ksp = 3.9 × 10−16

c. PbS, Ksp = 8.4 × 10−28

Solid lead nitrate is added slowly to a solution that is 0.010 M in sodium sulfate and 0.010 M in sodium chromate at 25°C. What percent of the chromate ions remain in solution, i.e., unprecipitated, just before lead sulfate begins to precipitate? Ksp for PbSO4 = 1.8 × 10−8, Ksp for PbCrO4 = 1.8 × 10−14 a. 0.18% b. 0.018% c. 0.0018% d. 0.00010% e. 0.00018%

d. 0.00010%

Solid Na2SO4 is added to a solution that is 0.30 M in both Sr2+ and Pb2+. Assuming no volume change, what will be the [Pb2+] at the point at which SrSO4 just begins to precipitate at 25°C? Ksp for SrSO4 = 2.8 × 10−7 and for PbSO4 = 1.8 × 10−8. a. 0.24 M b. 0.16 M c. 0.30 M d. 0.019 M e. 0.040 M

d. 0.019 M

If solid AgNO3 is slowly added to a solution that is 0.050 M in NaI and 0.12 M in NaCl, what is the concentration of I− when AgCl just begins to precipitate? Ksp for AgCl = 1.8 × 10−10, Ksp for AgI = 1.5 × 10−16 a. 1.0 × 10^−9 M b. 9.2 × 10^−9 M c. 8.5 × 10^−8 M d. 1.0 × 10^−7 M e. 6.7 × 10^−7 M

d. 1.0 × 10^−7 M

What concentration of aqueous NH3 is necessary to just start precipitation of Mn(OH)2 from a 0.020 M solution MnSO4? Kb for NH3 is 1.8 × 10−5 and Ksp for Mn(OH)2 is 4.6 × 10−14. a. 1.4 × 10^−5 M b. 3.7 × 10^−7 M c. 1.6 × 10^−6 M d. 1.3 × 10^−7 M e. 8.4 × 10^−2 M

d. 1.3 × 10^−7 M

The solubility of Fe(OH)2 is 3.00 × 10−3 g in 2.00 liters at 18°C. What is its Ksp at 18°C? a. 4.92 × 10^−12 b. 6.03 × 10^−9 c. 2.44 × 10^−10 d. 1.86 × 10^−14 e. 2.11 × 10^−11

d. 1.86 × 10^−14

Calculate the concentration of cyanide ions in a 0.10 M [Cd(CN)4]2− solution. The complex ion dissociates: [Cd(CN)4]2− Cd2+ + 4CN− and its dissociation constant is 7.8 × 10−18. a. 1.1 × 10^−4 M b. 7.9 × 10^−5 M c. 9.4 × 10^−6 M d. 3.2 × 10^−4 M e. 8.8 × 10^−4 M

d. 3.2 × 10^−4 M

Ksp for lead fluoride is 3.7 × 10−8. What is the molar solubility of PbF2 in 0.10 M NaF? a. 4.6 × 10^−5 M b. 1.9 × 10^−4 M c. 3.7 × 10^−7 M d. 3.7 × 10^−6 M e. 8.5 × 10^−8 M

d. 3.7 × 10^−6 M

How many grams of MgF2 will dissolve in 150. mL of 0.100 M NaF solution? Ksp for MgF2 = 6.4 × 10−9 a. 6.2 × 10^−7 g b. 4.1 × 10^−6 g c. 1.0 × 10^−5 g d. 6.0 × 10^−6 g e. 9.3 × 10^−7 g

d. 6.0 × 10^−6 g

Calculate the [Ca2+] required to start the precipitation of calcium fluoride, CaF2, from a solution containing 0.0025 M F− at 25°C. Ksp for CaF2 = 3.9 × 10−11. a. 6.4 × 10^−7 M b. 5.2 × 10^−10 M c. 4.8 × 10^−3 M d. 6.2 × 10^−6 M e. 1.6 × 10^−8 M

d. 6.2 × 10^−6 M

A solution is 1.0 × 10−4 M in sodium sulfate, Na2SO4, and 1.0 × 10−4 M in sodium selenate, Na2SeO4. Solid barium chloride, BaCl2, is added slowly and one of the two salts, BaSO4 or BaSeO4, begins to precipitate. What percentage of the anion that precipitates first has precipitated at the point at which the second anion begins to precipitate? Ksp for BaSO4 is 1.1 × 10−10 and for BaSeO4 is 2.8 × 10−11. a. 10% b. 25% c. 90% d. 75% e. 50%

d. 75%

What is the minimum concentration of Ni2+ required to begin precipitating Ni(OH)2(s) in a solution of pH 10.20? For Ni(OH)2, Ksp = 2.0 × 10-15. a. 7.9 × 10^-5 M b. 3.2 × 10^-5 M c. 1.3 × 10^-11 M d. 8.0 × 10^-8 M e. 1.9 × 10^-17 M

d. 8.0 × 10^-8 M

The solubility product for barium chromate, BaCrO4, is 2.0 × 10−10 and the solubility product for lead chromate, PbCrO4, is 1.8 × 10−14. If solid Na2CrO4 is added slowly to a solution which is 0.010 M in Ba(NO3)2 and 0.010 M in Pb(NO3)2, what will the concentration of Pb2+ be just before BaCrO4 begins to precipitate? Assume no volume change due to the addition of solid Na2CrO4. a. 4.0 × 10^−7 M b. 2.0 × 10^−8 M c. 1.8 × 10^−14 M d. 9.0 × 10^−7 M e. 1.4 × 10^−5 M

d. 9.0 × 10^−7 M

What is the pH of a saturated solution of Fe(OH)2? For Fe(OH)2, Ksp = 8.0 × 10-16. a. 4.93 b. 8.77 c. 5.23 d. 9.07 e. 7.00

d. 9.07

Solid AgNO3 is added slowly to a solution which is 0.0010 M in NaCl and 0.0010 M in NaBr. The Ksp for AgCl is 1.8 × 10−10 and the Ksp for AgBr is 3.3 × 10−13. What concentration of Br− remains in solution when 50.% of the Cl− has precipitated? a. 3.6 × 10^−7 M b. 1.2 × 10^−8 M c. 3.3 × 10^−10 M d. 9.2 × 10^−7 M e. 4.2 × 10^−9 M

d. 9.2 × 10^−7 M

A 4.0 × 10-4 M solution of MnSO4 is gradually made more basic by adding NaOH. At what pH will manganese(II) hydroxide begin to precipitate? For Mn(OH)2, Ksp = 2.0 × 10-13. a. 4.70 b. 9.57 c. 4.65 d. 9.35 e. 9.30

d. 9.35

If the molar solubility of manganese(II) hydroxide, Mn(OH)2 is 2.26 x 10-5 M, what is the pH of a saturated solution of manganese(II) hydroxide? a. 11.978 b. 11.677 c. 10.479 d. 9.655 e. 9.354

d. 9.655

An aqueous solution of silver bromide is adjusted so that the concentration of silver ion in solution is limited to a maximum of 1.0 × 10−9 M. Which of the following statements about the solution is false? Ksp for AgBr is 3.3 × 10−13. a. The minimum concentration of bromide needed for this limit is 3.3 × 10−4 M. b. If the concentration of bromide is 1.5 × 10−6, no precipitate will form. c. If the concentration of bromide is held precisely at 3.3 × 10−4, neither forward nor reverse process is favored. d. Adjusting the bromide concentration always effects the silver concentration. e. If [Br−] is raised to 1 × 10−3 M, the silver concentration drops to 3.3 × 10−10.

d. Adjusting the bromide concentration always effects the silver concentration.

If a solution of 0.10 M HCN is mixed with a solution of 0.10 M AgNO3, what possible precipitate may form? a. Ag2CN b. NH4NO3 c. NH4OH d. AgCN e. None is possible.

d. AgCN

Which of the following is a technique that could increase the solubility of CuS? a. Reducing the S2− to sulfur by adding nitric acid. b. Conversion of S2− to H2S by adding HCl. c. Conversion of Cu2+ to a complex ion by adding NH3. d. All three would increase the solubility. e. None of these would increase the solubility.

d. All three would increase the solubility.

We mix each of the following pairs of solutions together. In which case would we not expect a precipitate (solid) to be formed? a. KCl solution and AgNO3 solution b. Pb(NO3)2 solution and H2SO4 solution c. CuCl2 solution and Na2S solution d. CaCl2 solution and HNO3 solution e. A precipitate would be likely to form in every case.

d. CaCl2 solution and HNO3 solution

If X = the molar solubility (mol/L) of Ca3(PO4)2, which of the following represents the correct relationship between the Ksp and X, the molar solubility of Ca3(PO4)2? a. Ksp = X^2 b. Ksp = 27 X^5 c. Ksp = 4 X^2 d. Ksp = 108 X^5 e. Ksp = 16 X^3

d. Ksp = 108 X^5

The Ksp for Fe(IO3)3 is 10−14. We mix two solutions, one containing Fe3+ and one containing IO3− ions at 25°C. At the instant of mixing, [Fe3+] = 10−2 M and [IO3−] = 10−5 M. Which one of the following statements is true? a. A precipitate forms, because Qsp > Ksp. b. A precipitate forms, because Qsp < Ksp. c. No precipitate forms, because Qsp > Ksp. d. No precipitate forms, because Qsp < Ksp. e. None of these statements is true.

d. No precipitate forms, because Qsp < Ksp.

Which of the following salts would not be expected to be more soluble in acidic solution than in pure water? a. Mg(OH)2 b. ZnS c. BaCO3 d. PbI2 e. AgF

d. PbI2

A solution is 0.012 M in Pb(NO3)2 and 0.20 M in Sr(NO3)2. Solid Na2SO4 is added until a precipitate just begins to form. The precipitate is ____ and the concentration of sulfate ion at this point is ____. Ksp for PbSO4 is 1.8 × 10−8 and for SrSO4 is 2.8 × 10−7. a. SrSO4; 2.6 × 10^−7 M b. SrSO4; 8.3 × 10^−7 M c. PbSO4; 6.3 × 10^−6 M d. PbSO4; 1.5 × 10^−6 M e. SrSO4; 1.4 × 10^−6 M

d. PbSO4; 1.5 × 10^−6 M

Calculate Q, the reaction quotient, for when 12.0mL of 4.38 x 10-4M Ba(C2H3O2)2 is mixed with 25.0mL of 2.67 x 10-5M Na3PO4, and predict whether a precipitate will form. Ksp for Ba3(PO4)2 is 3.40 x 10-23 a. Q = 3.16 x 10^-10 and a precipitate will form b. Q = 1.75 x 10^-24 and a precipitate will form c. Q = 3.16 x 10^-10 and no precipitate will form d. Q = 1.75 x 10^-24 and no precipitate will form e. Q = 3.40 x 10^-23 and it is exactly at equilibrium

d. Q = 1.75 x 10^-24 and no precipitate will form

When 10.0 g Na2CO3 is added to 1.0 L of a solution containing 0.05 M of each Mg2+, Ca2+, Sr2+, and Ba2+, which cation concentration is lowest after the carbonate salts precipitate? = 4.0 × 10−5, = 4.8 × 10−9, = 9.4 × 10−10, = 8.1 × 10−9 a. Mg2+ b. Ca2+ c. Na+ d. Sr2+ e. Ba2+

d. Sr2+

Which statement about solubility product constant, Ksp, is false? a. It is a constant at a given temperature. b. It equals the equilibrium constant in equilibria that involve slightly soluble compounds in water. c. The concentration of the solid is not included in the solubility product expression. d. The solubility product expression is the product of the concentrations of the compound's constituent ions. e. It is based on the solubility product principle.

d. The solubility product expression is the product of the concentrations of the compound's constituent ions.

Which of the following solubility product expressions is incorrect? Compound / Ksp Expression a. gold(III) chloride / [Au3+][Cl−]3 b. calcium fluoride / [Ca2+][F−]2 c. lead(II) iodide / [Pb2+][I−]2 d. zinc phosphate / [Zn2+][PO43−] e. silver chromate / [Ag+]2[CrO42−]

d. zinc phosphate / [Zn2+][PO43−]

What mass of CaF2 is contained in 1.0 liter of saturated solution? Ksp = 3.9 × 10−11. a. 0.0010 g b. 0.0028 g c. 0.0034 g d. 0.010 g e. 0.017 g

e. 0.017 g

If 1.0 liter of solution is to be made 0.010 M in Mg(NO3)2 and 0.10 M in aqueous ammonia, how many moles of NH4Cl are necessary to prevent the precipitation of magnesium hydroxide? The solubility product for Mg(OH)2 is 1.5 × 10−11, and the ionization constant for aqueous ammonia is 1.8 × 10−5. a. 0.018 mol b. 0.016 mol c. 0.020 mol d. 0.040 mol e. 0.046 mol

e. 0.046 mol

A solution is 0.0010 M in both Ag+ and Au+. Some solid NaCl is added slowly until the second solid compound just begins to precipitate. What is the concentration of Au+ ions at this point? Ksp for AgCl = 1.8 × 10−10 and for AuCl is 2.0 × 10−13. a. 2.0 × 10^−10 M b. 4.5 × 10^−7 M c. 1.8 × 10^−7 M d. 3.0 × 10^−4 M e. 1.1 × 10^−6 M

e. 1.1 × 10^−6 M

Magnesium hydroxide is a slightly soluble substance. If the pH of a saturated solution of Mg(OH)2 is 10.49 at 25°C, calculate Ksp for Mg(OH)2. a. 8.8 × 10^−16 b. 4.2 × 10^−15 c. 6.0 × 10^−10 d. 4.4 × 10^−14 e. 1.5 × 10^−11

e. 1.5 × 10^−11

Calculate the solubility product constant for aluminum hydroxide. Its molar solubility is 2.9 × 10−9 mole per liter at 25°C. a. 9.8 × 10^−26 b. 4.9 × 10^−26 c. 7.1 × 10^−35 d. 2.1 × 10^−34 e. 1.9 × 10^−33

e. 1.9 × 10^−33

Calculate the concentration of OH− ions in a saturated Mn(OH)2 solution. The solubility product for Mn(OH)2 is 4.6 × 10−14. a. 1.0 × 10^−5 M b. 2.0 × 10^−5 M c. 1.6 × 10^−5 M d. 3.2 × 10^−5 M e. 4.5 × 10^−5 M

e. 4.5 × 10^−5 M

A 50.0 mL-sample of 1.8 M aqueous NH3 is mixed with an equal volume of a solution containing 0.010 mol of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent precipitation of Mg(OH)2? Ksp for Mg(OH)2 = 1.5 × 10−11 and Kb for NH3 = 1.8 × 10−5. a. 4.4 g b. 5.7 g c. 6.2 g d. 6.6 g e. 7.1 g

e. 7.1 g

How many grams of BaCO3 will dissolve in 853 mL of 0.15 M BaCl2? = 8.1 × 10−9 a. 1.1 × 10^−5 g b. 4.6 × 10^−8 g c. 5.5 × 10^−8 g d. 8.1 × 10^−9 g e. 9.1 × 10^−6 g

e. 9.1 × 10^−6 g

What is the minimum concentration of iodide ion required to limit the concentration of lead ion in solution to a maximum of 1.0 × 10−6 M? Ksp for PbI2 is 8.7 × 10−9. a. 1.7 × 10^−2 M b. 1.8 × 10^−1 M c. 7.6 × 10^−5 M d. 8.7 × 10^−3 M e. 9.3 × 10^−2 M

e. 9.3 × 10^−2 M

Calculate the pH in a saturated Mn(OH)2 solution. The solubility product for Mn(OH)2 is 4.6 × 10−14. a. 9.00 b. 9.25 c. 9.35 d. 9.50 e. 9.65

e. 9.65

Which of the following responses contains all of the true statements? I. An ion may never be completely precipitated from solution, even when the precipitating reagent is used in large excess. II. If solid NaCl is added slowly to a saturated solution of NiS in contact with solid NiS, nothing significant will happen to the NiS. III. Consider two relatively insoluble 1:1 salts (i.e., one cation and one anion per formula unit) containing the same cation, whose solubility products differ by 104. More than 90% of one anion can be precipitated before the other precipitates when the common cation is added to a solution of the two anions. a. I and III b. I and II c. II and III d. III e. I, II, and III

e. I, II, and III

If aqueous solutions of the following pairs of compounds are mixed, which combination might result in the formation of a precipitate? a. MgCl2 + Na2S b. NH4ClO4 + K2S c. BaCl2 + Ca(CH3COO)2 d. CrCl3 + Ni(NO3)2 e. Na3PO4 + Cr(NO3)3

e. Na3PO4 + Cr(NO3)3

How might one test if PbS has been completely precipitated from a saturated H2S solution? a. heat the solution b. add a strong acid c. add a weak acid d. add more H2S e. add a weak base

e. add a weak base

The cations in many slightly soluble compounds can form complex ions; this results in the ____ of the slightly soluble compound as ____ are formed with molecules and ions such as NH3, CN−, and the halides. a. precipitation; weak electrolytes b. dissolution; weak electrolytes c. dissolution; ions d. precipitation; coordinate covalent bonds e. dissolution; coordinate covalent bonds

e. dissolution; coordinate covalent bonds