The solubility product constant of Mg(OH)2 is 9.0 × 10-12.If an aqueous solution is 0.010 M with respect to Mg2+ ion,the amount of [OH-] required to start the precipitation of Mg(OH)2(s)is:

A) 1.5 × 10-7 M B) 3.0 × 10-5 M C) 3.0 × 10-7 M D) 9.0 × 10-10 M E) 1.5 × 10-5 M A) 1.5 × 10-7 M B) 3.0 × 10-5 M C) 3.0 × 10-7 M D) 9.0 × 10-10 M E) 1.5 × 10-5 M

Fe(OH)3 is most soluble in which aqueous solution?

A) 0.2 M HCl B) 0.1 M KOH C) pure water D) 0.1 M FeCl3 E) 0.2 M CaCl2 A) 0.2 M HCl B) 0.1 M KOH C) pure water D) 0.1 M FeCl3 E) 0.2 M CaCl2

When 200 mL of 0.10 M BaCl2(aq)is added to 100 mL of 0.30 M Na2SO4(aq),the number of moles of BaSO4 (solubility product = 1.1 × 10-10)precipitated is ________.

A) 0.020 mol B) 0.010 mol C) 0.20 mol D) 0.030 mol E) 0.10 mol A) 0.020 mol B) 0.010 mol C) 0.20 mol D) 0.030 mol E) 0.10 mol

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

What is the approximate concentration of free Fe3+(aq)ion in a solution prepared by mixing equal volumes of 0.06 M Fe3+(aq)and 4.0 M F-(aq)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

The solubility product constant of M2CrO4(s)is 7.11 × 10-15.How many moles of M2CrO4(s)will dissolve in 744 mL of aqueous solution in which [CrO42-] = 0.056 M?

A) 2.7 × 10-7 mol B) 1.8 × 10-7 mol C) 1.2 × 10-5 mol D) 9.0 × 10-5 mol E) 3.6 × 10-7 mol A) 2.7 × 10-7 mol B) 1.8 × 10-7 mol C) 1.2 × 10-5 mol D) 9.0 × 10-5 mol E) 3.6 × 10-7 mol

What is the molar solubility of Mg(OH)2(s)in a basic aqueous solution with a pH of 12.50? Ksp for Mg(OH)2(s)is

A) 1.8 × 10-10 mol L-1 B) 5.6 × 10-9 mol L-1 C) 2.4 × 10-6 mol L-1 D) 1.1 × 10-4 mol L-1 A) 1.8 × 10-10 mol L-1 B) 5.6 × 10-9 mol L-1 C) 2.4 × 10-6 mol L-1 D) 1.1 × 10-4 mol L-1

The molar solubility of SrSO4 (Ksp = 7.6 × 10-7)is:

A) 2.8 × 10-5 M B) 7.6 × 10-7 M C) 8.7 × 10-8 M D) 8.7 × 10-4 M E) 9.1 × 10-3 M A) 2.8 × 10-5 M B) 7.6 × 10-7 M C) 8.7 × 10-8 M D) 8.7 × 10-4 M E) 9.1 × 10-3 M

Exam 18: Solubility and Complex-Ion Equilibria

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The solubility product constant of PbI₂(s)is 7.1 × 10^-9.How many moles of PbI₂ will precipitate if 250 mL of a 0.200 M solution of NaI(aq)are added to 150 mL of 0.100 M solution of Pb(NO₃)₂(aq)? You may neglect hydrolysis.

(Multiple Choice)

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Question 21

The solubility product constant of Mg(OH)₂ is 9.0 × 10^-12.If an aqueous solution is 0.010 M with respect to Mg²⁺ ion,the amount of [OH^-] required to start the precipitation of Mg(OH)₂(s)is:

(Multiple Choice)

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Question 22

Fe(OH)₃ is most soluble in which aqueous solution?

(Multiple Choice)

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Question 23

When equal volumes of the indicated aqueous solutions are mixed,precipitation should occur only for:

(Multiple Choice)

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Question 24

When 200 mL of 0.10 M BaCl₂(aq)is added to 100 mL of 0.30 M Na₂SO₄(aq),the number of moles of BaSO₄(solubility product = 1.1 × 10^-10)precipitated is ________.

(Multiple Choice)

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Question 25

The K_sp of AgCl is 1.7 × 10^-10.How many moles of MnCl₂ can be dissolved in one liter of an aqueous solution in which [AgNO₃] = 3.4 × 10^-4 M before a precipitate appears?

(Multiple Choice)

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Question 26

Calculate the solubility (in g L^-1)of calcium fluoride in water at 25 °C if the K_sp for CaF₂ Is 1.5 × 10^-10

(Multiple Choice)

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Question 27

A concentrated buffer of pH 8.0 is added to an equal volume of an aqueous solution that is 0.080 M in each of the ions Zn²⁺,Ni²⁺,and Mn²⁺.The expected precipitate would consist of ________.

(Multiple Choice)

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Question 28

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

(Multiple Choice)

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Question 29

Which of the following soil additives would best reduce the concentration of dissolved Fe³⁺ in ground water?

(Multiple Choice)

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Question 30

What is the minimum concentration of CN^-(aq)that will prevent the precipitation of AgX(s)from a solution that is 0.149 M in X^-(aq)and 0.0184 M in Ag⁺(aq)? (K_sp for AgX(s)= 5.2 × 10^-17;K_f for Ag(CN)₂^- = 5.6 × 10¹⁸)

(Multiple Choice)

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Question 31

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

(Multiple Choice)

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Question 32

Which of the following has the largest molar solubility?

(Multiple Choice)

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Question 33

The solubility of CaF₂ is 0.00021 mole per liter.What is the solubility product constant for CaF₂?

(Multiple Choice)

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Question 34

Predict the molar solubility of the following salt in an aqueous solution that contains the given concentration of one of its ions: AgI;[I^-] = 7.2 × 10^-6 M;K_sp = 8.5 × 10^-17

(Multiple Choice)

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Question 35

The solubility product constant of M₂CrO₄(s)is 7.11 × 10^-15.How many moles of M₂CrO₄(s)will dissolve in 744 mL of aqueous solution in which [CrO₄^2-] = 0.056 M?

(Multiple Choice)

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Question 36

What is the molar solubility of Mg(OH)₂(s)in a basic aqueous solution with a pH of 12.50? K_spfor Mg(OH)₂(s)is

(Multiple Choice)

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Question 37

Write the solubility product constant expression for the following salt: PbC₂O₄(s).

(Multiple Choice)

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Question 38

What is the molar solubility of barium carbonate in pure water? (K_sp = 5.1 × 10^-9)

(Multiple Choice)

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Question 39

The molar solubility of SrSO₄ (K_sp = 7.6 × 10^-7)is:

(Multiple Choice)

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Question 40

Showing 21 - 40 of 104

Exam 18: Solubility and Complex-Ion Equilibria

The solubility product constant of PbI2(s)is 7.1 × 10-9.How many moles of PbI2 will precipitate if 250 mL of a 0.200 M solution of NaI(aq)are added to 150 mL of 0.100 M solution of Pb(NO3)2(aq)? You may neglect hydrolysis.

The solubility product constant of Mg(OH)2 is 9.0 × 10-12.If an aqueous solution is 0.010 M with respect to Mg2+ ion,the amount of [OH-] required to start the precipitation of Mg(OH)2(s)is:

Fe(OH)3 is most soluble in which aqueous solution?

When equal volumes of the indicated aqueous solutions are mixed,precipitation should occur only for:

When 200 mL of 0.10 M BaCl2(aq)is added to 100 mL of 0.30 M Na2SO4(aq),the number of moles of BaSO4 (solubility product = 1.1 × 10-10)precipitated is ________.

The Ksp of AgCl is 1.7 × 10-10.How many moles of MnCl2 can be dissolved in one liter of an aqueous solution in which [AgNO3] = 3.4 × 10-4 M before a precipitate appears?

Calculate the solubility (in g L-1)of calcium fluoride in water at 25 °C if the Ksp for CaF2 Is 1.5 × 10-10

A concentrated buffer of pH 8.0 is added to an equal volume of an aqueous solution that is 0.080 M in each of the ions Zn2+,Ni2+,and Mn2+.The expected precipitate would consist of ________.

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

Which of the following soil additives would best reduce the concentration of dissolved Fe3+ in ground water?

What is the minimum concentration of CN-(aq)that will prevent the precipitation of AgX(s)from a solution that is 0.149 M in X-(aq)and 0.0184 M in Ag+(aq)? (Ksp for AgX(s)= 5.2 × 10-17;Kf for Ag(CN)2- = 5.6 × 1018)

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

Which of the following has the largest molar solubility?

The solubility of CaF2 is 0.00021 mole per liter.What is the solubility product constant for CaF2?

Predict the molar solubility of the following salt in an aqueous solution that contains the given concentration of one of its ions: AgI;[I-] = 7.2 × 10-6 M;Ksp = 8.5 × 10-17

The solubility product constant of M2CrO4(s)is 7.11 × 10-15.How many moles of M2CrO4(s)will dissolve in 744 mL of aqueous solution in which [CrO42-] = 0.056 M?

What is the molar solubility of Mg(OH)2(s)in a basic aqueous solution with a pH of 12.50? Ksp for Mg(OH)2(s)is

Write the solubility product constant expression for the following salt: PbC2O4(s).

What is the molar solubility of barium carbonate in pure water? (Ksp = 5.1 × 10-9)

The molar solubility of SrSO4 (Ksp = 7.6 × 10-7)is:

Matter: Its Properties and Measurement

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Principles of Chemical Equilibrium

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The solubility product constant of PbI₂(s)is 7.1 × 10^-9.How many moles of PbI₂ will precipitate if 250 mL of a 0.200 M solution of NaI(aq)are added to 150 mL of 0.100 M solution of Pb(NO₃)₂(aq)? You may neglect hydrolysis.

The solubility product constant of Mg(OH)₂ is 9.0 × 10^-12.If an aqueous solution is 0.010 M with respect to Mg²⁺ ion,the amount of [OH^-] required to start the precipitation of Mg(OH)₂(s)is:

Fe(OH)₃ is most soluble in which aqueous solution?

When 200 mL of 0.10 M BaCl₂(aq)is added to 100 mL of 0.30 M Na₂SO₄(aq),the number of moles of BaSO₄(solubility product = 1.1 × 10^-10)precipitated is ________.

The K_sp of AgCl is 1.7 × 10^-10.How many moles of MnCl₂ can be dissolved in one liter of an aqueous solution in which [AgNO₃] = 3.4 × 10^-4 M before a precipitate appears?

Calculate the solubility (in g L^-1)of calcium fluoride in water at 25 °C if the K_sp for CaF₂ Is 1.5 × 10^-10

A concentrated buffer of pH 8.0 is added to an equal volume of an aqueous solution that is 0.080 M in each of the ions Zn²⁺,Ni²⁺,and Mn²⁺.The expected precipitate would consist of ________.

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

Which of the following soil additives would best reduce the concentration of dissolved Fe³⁺ in ground water?

What is the minimum concentration of CN^-(aq)that will prevent the precipitation of AgX(s)from a solution that is 0.149 M in X^-(aq)and 0.0184 M in Ag⁺(aq)? (K_sp for AgX(s)= 5.2 × 10^-17;K_f for Ag(CN)₂^- = 5.6 × 10¹⁸)

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

The solubility of CaF₂ is 0.00021 mole per liter.What is the solubility product constant for CaF₂?

Predict the molar solubility of the following salt in an aqueous solution that contains the given concentration of one of its ions: AgI;[I^-] = 7.2 × 10^-6 M;K_sp = 8.5 × 10^-17

The solubility product constant of M₂CrO₄(s)is 7.11 × 10^-15.How many moles of M₂CrO₄(s)will dissolve in 744 mL of aqueous solution in which [CrO₄^2-] = 0.056 M?

What is the molar solubility of Mg(OH)₂(s)in a basic aqueous solution with a pH of 12.50? K_spfor Mg(OH)₂(s)is

Write the solubility product constant expression for the following salt: PbC₂O₄(s).

What is the molar solubility of barium carbonate in pure water? (K_sp = 5.1 × 10^-9)

The molar solubility of SrSO₄ (K_sp = 7.6 × 10^-7)is: