The solubility of copper(II) iodate Cu(IO3)2 is reported as 0.12 g per 100 mL. What is the solubility product constant for this salt?

A) 9.8 × 10-8 B) 8.6 × 10-7 C) 7.3 × 10-6 D) 6.4 × 10-5 E) 1.2 × 10-4 A) 9.8 × 10-8 B) 8.6 × 10-7 C) 7.3 × 10-6 D) 6.4 × 10-5 E) 1.2 × 10-4

The solubility product constant of Li3PO4 is 3.2 × 10-9. What is the molar solubility of Li3PO4 in water?

A) 3.3 × 10-3 M B) 9.3 × 10-4 M C) 7.5 × 10-3 M D) 1.5 × 10-3 M E) 5.7 × 10-5 M A) 3.3 × 10-3 M B) 9.3 × 10-4 M C) 7.5 × 10-3 M D) 1.5 × 10-3 M E) 5.7 × 10-5 M

To a concentrated buffer of pH 9.0 was added an equal volume of a solution that was 0.20 M in each of the ions Ca2+, Cd2+, and Cu2+. The expected precipitate would consist of: salt: calcium hydroxide cadmium hydroxide copper(II) hydroxide Ksp: 4.0 × 10-6 &emsp; 2.0 × 10-14 &emsp; 1.8 × 10-19

A) only Ca(OH)2 B) only Cd(OH)2 C) only Cu(OH)2 D) only Cd(OH)2 and Cu(OH)2 E) Ca(OH)2, Cd(OH)2, and Cu(OH)2 A) only Ca(OH)2 B) only Cd(OH)2 C) only Cu(OH)2 D) only Cd(OH)2 and Cu(OH)2 E) Ca(OH)2, Cd(OH)2, and Cu(OH)2

What is the approximate concentration of free Fe3+ ion in a solution prepared by mixing equal volumes of 0.06 M Fe3+ and 4.0 M F- solutions? [The net formation constant for FeF5(H2O)2- is 2.0 × 1015.]

A) 2.8 × 10-23 M B) 6.7 × 10-21 M C) 6.9 × 10-19 M D) 4.0 × 10-15 M E) 8.9 × 10-10 M A) 2.8 × 10-23 M B) 6.7 × 10-21 M C) 6.9 × 10-19 M D) 4.0 × 10-15 M E) 8.9 × 10-10 M

Write the solubility product constant for KAl(SO4)2(s)?

A) ([K+] × [Al3+] × 2[SO42-]/[KAl(SO4)2]) B) ([K+] × [Al3+] × [SO42-]/[KAl(SO4)2]) C) ([K+] × [Al3+] × [SO42-]) D) ([K+] × [Al3+] × [SO42-]2) E) none of these A) ([K+] × [Al3+] × 2[SO42-]/[KAl(SO4)2]) B) ([K+] × [Al3+] × [SO42-]/[KAl(SO4)2]) C) ([K+] × [Al3+] × [SO42-]) D) ([K+] × [Al3+] × [SO42-]2) E) none of these

Exam 18: Solubility and Complex-Ion Equilibria

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When 100 mL each of 2.0 × 10^-6 M Ag+ and 2.0 × 10^-3 M Br- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10^-13.

(Multiple Choice)

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Question 81

The solubility of copper(II) iodate Cu(IO₃)₂ is reported as 0.12 g per 100 mL. What is the solubility product constant for this salt?

(Multiple Choice)

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Question 82

The following table lists five compounds and their Ksp value. Which is least soluble? ZnS 2 × 10^-25 TlBr 3.4 × 10^-6 AgCl 1.8 × 10^-10 FeS 6 × 10^-19 CuI 1.1 × 10^-12

(Multiple Choice)

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Question 83

Consider an aqueous solution which is 0.020 M in Pb2+ and 0.20 M in Ag+. Concentrated potassium iodide solution (so that volume changes may be neglected) is added gradually with good stirring to this solution. Eventually the iodide ion concentration should increase enough to cause precipitation of the second ion. What will be the concentration of the ion that precipitates first when the second ion just begins to precipitate?

(Multiple Choice)

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Question 84

The solubility product constant of Li₃PO₄ is 3.2 × 10^-9. What is the molar solubility of Li₃PO₄ in water?

(Multiple Choice)

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Question 85

To a concentrated buffer of pH 9.0 was added an equal volume of a solution that was 0.20 M in each of the ions Ca²⁺, Cd²⁺, and Cu²⁺. The expected precipitate would consist of: salt: calcium hydroxide cadmium hydroxide copper(II) hydroxide Ksp: 4.0 × 10^-6 2.0 × 10^-14 1.8 × 10^-19

(Multiple Choice)

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Question 86

What is the approximate concentration of free Fe³⁺ ion in a solution prepared by mixing equal volumes of 0.06 M Fe³⁺ and 4.0 M F- solutions? [The net formation constant for FeF₅(H₂O)₂^- is 2.0 × 10¹⁵.]

(Multiple Choice)

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Question 87

Write the solubility product constant expression for the following salt: Ca₃(PO₄)₂.

(Multiple Choice)

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Question 88

A saturated solution of magnesium fluoride has a concentration of 1.17 × 10^-3 M. For this compound, Ksp =

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Question 89

To a saturated solution of barium carbonate is added just enough sodium sulfate to achieve a maximum sulfate concentration without precipitation of barium sulfate. If no complexes form and the "salt effect" is negligible, what is the concentration of the sulfate ion in this solution? [Ksp for barium carbonate is 1.6 × 10^-9; Ksp for barium sulfate is 7.9 × 10^-11]

(Multiple Choice)

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Question 90

Write the solubility product constant expression for the following salt: Na₂CO₃.

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Question 91

Qualitative cation analysis has been replaced in recent years by instrumental analysis.

(True/False)

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Question 92

Equal volumes of 0.020 M Ag⁺ solution and 2.0 M NH₃ solution are mixed. Kf for [Ag(NH₃)₂]+ is 1.6 × 107. If trisodium arsenate is added so that the arsenate ion concentration is 0.10 M, will silver arsenate precipitate? What is Q? Ksp for silver arsenate is 1.0 × 10^-22.

(Multiple Choice)

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Question 93

Write the solubility product constant for KAl(SO₄)₂(s)?

(Multiple Choice)

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Question 94

Concentrated solutions of copper (I) nitrate, sodium sulfate and silver acetate are mixed together. The precipitate which forms is ________.

(Multiple Choice)

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Question 95

Showing 81 - 95 of 95

Exam 18: Solubility and Complex-Ion Equilibria

When 100 mL each of 2.0 × 10-6 M Ag+ and 2.0 × 10-3 M Br- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10-13.

The solubility of copper(II) iodate Cu(IO3)2 is reported as 0.12 g per 100 mL. What is the solubility product constant for this salt?

The following table lists five compounds and their Ksp value. Which is least soluble? ZnS 2 × 10-25 TlBr 3.4 × 10-6 AgCl 1.8 × 10-10 FeS 6 × 10-19 CuI 1.1 × 10-12

The solubility product constant of Li3PO4 is 3.2 × 10-9. What is the molar solubility of Li3PO4 in water?

To a concentrated buffer of pH 9.0 was added an equal volume of a solution that was 0.20 M in each of the ions Ca2+, Cd2+, and Cu2+. The expected precipitate would consist of: salt: calcium hydroxide cadmium hydroxide copper(II) hydroxide Ksp: 4.0 × 10-6 2.0 × 10-14 1.8 × 10-19

What is the approximate concentration of free Fe3+ ion in a solution prepared by mixing equal volumes of 0.06 M Fe3+ and 4.0 M F- solutions? [The net formation constant for FeF5(H2O)2- is 2.0 × 1015.]

Write the solubility product constant expression for the following salt: Ca3(PO4)2.

A saturated solution of magnesium fluoride has a concentration of 1.17 × 10-3 M. For this compound, Ksp =

Write the solubility product constant expression for the following salt: Na2CO3.

Qualitative cation analysis has been replaced in recent years by instrumental analysis.

Equal volumes of 0.020 M Ag+ solution and 2.0 M NH3 solution are mixed. Kf for [Ag(NH3)2]+ is 1.6 × 107. If trisodium arsenate is added so that the arsenate ion concentration is 0.10 M, will silver arsenate precipitate? What is Q? Ksp for silver arsenate is 1.0 × 10-22.

Write the solubility product constant for KAl(SO4)2(s)?

Concentrated solutions of copper (I) nitrate, sodium sulfate and silver acetate are mixed together. The precipitate which forms is ________.

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When 100 mL each of 2.0 × 10^-6 M Ag+ and 2.0 × 10^-3 M Br- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10^-13.

The solubility of copper(II) iodate Cu(IO₃)₂ is reported as 0.12 g per 100 mL. What is the solubility product constant for this salt?

The following table lists five compounds and their Ksp value. Which is least soluble? ZnS 2 × 10^-25 TlBr 3.4 × 10^-6 AgCl 1.8 × 10^-10 FeS 6 × 10^-19 CuI 1.1 × 10^-12

The solubility product constant of Li₃PO₄ is 3.2 × 10^-9. What is the molar solubility of Li₃PO₄ in water?

To a concentrated buffer of pH 9.0 was added an equal volume of a solution that was 0.20 M in each of the ions Ca²⁺, Cd²⁺, and Cu²⁺. The expected precipitate would consist of: salt: calcium hydroxide cadmium hydroxide copper(II) hydroxide Ksp: 4.0 × 10^-6 2.0 × 10^-14 1.8 × 10^-19

What is the approximate concentration of free Fe³⁺ ion in a solution prepared by mixing equal volumes of 0.06 M Fe³⁺ and 4.0 M F- solutions? [The net formation constant for FeF₅(H₂O)₂^- is 2.0 × 10¹⁵.]

Write the solubility product constant expression for the following salt: Ca₃(PO₄)₂.

A saturated solution of magnesium fluoride has a concentration of 1.17 × 10^-3 M. For this compound, Ksp =

Write the solubility product constant expression for the following salt: Na₂CO₃.

Equal volumes of 0.020 M Ag⁺ solution and 2.0 M NH₃ solution are mixed. Kf for [Ag(NH₃)₂]+ is 1.6 × 107. If trisodium arsenate is added so that the arsenate ion concentration is 0.10 M, will silver arsenate precipitate? What is Q? Ksp for silver arsenate is 1.0 × 10^-22.

Write the solubility product constant for KAl(SO₄)₂(s)?