Question 1

The pH of a saturated solution of Ca(OH)₂ is 12.37. What is the K_sp of Ca(OH)₂? ________

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Question 2

What is the molar solubility of Ca(OH)₂ in a 0.300 M NaOH solution? The K_sp of Ca(OH)₂ is 6.5 × 10^-6.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

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Question 3

What is the molar solubility of AgCl in a 0.450 M solution of KCl? The K_sp of AgCl is 1.8 × 10^-10.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

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Question 4

A student mixes 100.00 mL of 0.250 M MgSO₄ with 250.00 mL 0.100 M NaOH. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text.Hint: Find the concentration of each ion in the insoluble compound and use those to find Q.

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Question 5

The solubility product for chromium(III)fluoride is K_sp = 6.6 × 10^-11. Using this information, what is the molar solubility of chromium(III)fluoride?

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Question 6

Calculate the minimum concentration of Cr³⁺ that must be added to 0.085 M NaF in order to form a precipitate of chromium(III)fluoride. The solubility constant for CrF₃ is 6.6 × 10^-11.

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Question 7

Calculate the concentration of chloride ions in a saturated lead(II)chloride solution. The K_sp = 2.4 × 10^-4 for lead(II)chloride.

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Question 8

A student mixes 50.00 mL of 0.500 M NaCl with 75.00 mL of 0.200 M AgNO₃. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text.Hint: Find the concentration of each ion in the insoluble compound and use those to find Q.

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Question 9

The solubility of lead(II)iodide is 0.064 g/100 mL at 20°C. What is the solubility product constant for lead(II)iodide at this temperature?

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Question 10

200 mL of an aqueous solution contains 0.030 M concentrations of both Sr²⁺ and Ca²⁺. If 100 mL of 2.0 × 10^-3 M Na₂SO₄ is added to this solution will a precipitate form? If so, what will the precipitate be? The K_sp values for SrSO₄ and CaSO₄ are 2.4 × 10^-5 and 3.2 × 10^-7.Hint: Remember that the solutions are diluted.

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Question 11

Given the following information: What is the equilibrium constant for the reaction,MgCO₃(s)+ H⁺(aq) Mg²⁺(aq)+ HCO₃^-(aq)

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Question 12

For the H₂CO₃/ HCO₃/CO₃^2- system at room temperature K_a1 = 4.5 × 10^-⁷, whileK_a2 = 4.7 × 10^-11. The K_sp for BaCO₃ is 5.0 × 10^-9.Calculate the equilibrium constant for the reaction,BaCO₃(s)+ H⁺(aq) Ba²⁺(aq)+ HCO₃^-(aq)

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Question 13

Many metal sulfides have ________ solubilities.

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Question 14

Metal sulfides actually dissolve in water by ________ with water, not by releasing S^2- ions into water.

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Question 15

Metal cations in the chloride solubility group can be separated from other cations because they form ________ chloride compounds in a solution of HCl.

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Question 16

Group II and group III cations (acid-insoluble and base-insoluble sulfides)can be separated out by forming a precipitate of acid-insoluble cations at low ________.

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Question 17

200 mL of an aqueous solution contains 0.030 M concentrations of both Sr²⁺ and Ca²⁺. If 100 mL of 2.0 × 10^-5 M Na₂SO₄ is added to this solution will a precipitate form? If so, what will the precipitate be? The K_sp values for SrSO₄ and CaSO₄ are 2.4 × 10^-5 and 3.2 × 10^-7.Hint: Remember that the solutions are being diluted and use the diluted concentrations

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Question 18

200 mL of an aqueous solution contains 0.030 M concentrations of both Sr²⁺ and Ca²⁺. If 100 mL of 6.0 × 10^-3 M Na₂SO₄ is added to this solution will a precipitate form? If so, what will the precipitate be? The K_sp values for SrSO₄ and CaSO₄ are 2.4 × 10^-5 and 3.2 × 10^-7.Hint: Remember that the solutions are being diluted and use the diluted concentrations

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Question 19

200 mL of an aqueous solution contains 0.030 M concentrations of both Pb²⁺ and Ag⁺. If 100 mL of 6.0 × 10^-2 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The K_sp values for PbCl₂ and AgCl are 1.7 × 10^-5 and 1.8 × 10^-10.Hint: Remember that the solutions are being diluted and use the diluted concentrations.

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Question 20

200 mL of an aqueous solution contains 0.030 M concentrations of both Pb²⁺ and Ag⁺. If 100 mL of 0.20 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The K_sp values for PbCl₂ and AgCl are 1.7 × 10^-5 and 1.8 × 10^-10.Hint: Remember that the solutions are being diluted and use the diluted concentrations.

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Quiz 18: Solubility and Simultaneous Equilibria

The pH of a saturated solution of Ca(OH)2 is 12.37. What is the Ksp of Ca(OH)2? ________

What is the molar solubility of Ca(OH)2 in a 0.300 M NaOH solution? The Ksp of Ca(OH)2 is 6.5 × 10-6.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

What is the molar solubility of AgCl in a 0.450 M solution of KCl? The Ksp of AgCl is 1.8 × 10-10.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

A student mixes 100.00 mL of 0.250 M MgSO4 with 250.00 mL 0.100 M NaOH. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text.Hint: Find the concentration of each ion in the insoluble compound and use those to find Q.

The solubility product for chromium(III)fluoride is Ksp = 6.6 × 10-11. Using this information, what is the molar solubility of chromium(III)fluoride?

Calculate the minimum concentration of Cr3+ that must be added to 0.085 M NaF in order to form a precipitate of chromium(III)fluoride. The solubility constant for CrF3 is 6.6 × 10-11.

Calculate the concentration of chloride ions in a saturated lead(II)chloride solution. The Ksp = 2.4 × 10-4 for lead(II)chloride.

A student mixes 50.00 mL of 0.500 M NaCl with 75.00 mL of 0.200 M AgNO3. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text.Hint: Find the concentration of each ion in the insoluble compound and use those to find Q.

The solubility of lead(II)iodide is 0.064 g/100 mL at 20°C. What is the solubility product constant for lead(II)iodide at this temperature?

Given the following information: What is the equilibrium constant for the reaction,MgCO3(s)+ H+(aq) Mg2+(aq)+ HCO3-(aq)

For the H2CO3/ HCO3/CO32- system at room temperature Ka1 = 4.5 × 10-7, whileKa2 = 4.7 × 10-11. The Ksp for BaCO3 is 5.0 × 10-9.Calculate the equilibrium constant for the reaction,BaCO3(s)+ H+(aq) Ba2+(aq)+ HCO3-(aq)

Many metal sulfides have ________ solubilities.

Metal sulfides actually dissolve in water by ________ with water, not by releasing S2- ions into water.

Metal cations in the chloride solubility group can be separated from other cations because they form ________ chloride compounds in a solution of HCl.

Group II and group III cations (acid-insoluble and base-insoluble sulfides)can be separated out by forming a precipitate of acid-insoluble cations at low ________.

The pH of a saturated solution of Ca(OH)₂ is 12.37. What is the K_sp of Ca(OH)₂? ________

What is the molar solubility of Ca(OH)₂ in a 0.300 M NaOH solution? The K_sp of Ca(OH)₂ is 6.5 × 10^-6.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

What is the molar solubility of AgCl in a 0.450 M solution of KCl? The K_sp of AgCl is 1.8 × 10^-10.Hint: Be sure to account for the presence of a common ion. You should also be able to simplify the math.

A student mixes 100.00 mL of 0.250 M MgSO₄ with 250.00 mL 0.100 M NaOH. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text.Hint: Find the concentration of each ion in the insoluble compound and use those to find Q.

The solubility product for chromium(III)fluoride is K_sp = 6.6 × 10^-11. Using this information, what is the molar solubility of chromium(III)fluoride?

Calculate the minimum concentration of Cr³⁺ that must be added to 0.085 M NaF in order to form a precipitate of chromium(III)fluoride. The solubility constant for CrF₃ is 6.6 × 10^-11.

Calculate the concentration of chloride ions in a saturated lead(II)chloride solution. The K_sp = 2.4 × 10^-4 for lead(II)chloride.

A student mixes 50.00 mL of 0.500 M NaCl with 75.00 mL of 0.200 M AgNO₃. Will a precipitate form? What is the identity of the precipitate? Consult Table 17.1 in your text.Hint: Find the concentration of each ion in the insoluble compound and use those to find Q.

Given the following information: What is the equilibrium constant for the reaction,MgCO₃(s)+ H⁺(aq) Mg²⁺(aq)+ HCO₃^-(aq)

For the H₂CO₃/ HCO₃/CO₃^2- system at room temperature K_a1 = 4.5 × 10^-⁷, whileK_a2 = 4.7 × 10^-11. The K_sp for BaCO₃ is 5.0 × 10^-9.Calculate the equilibrium constant for the reaction,BaCO₃(s)+ H⁺(aq) Ba²⁺(aq)+ HCO₃^-(aq)

Metal sulfides actually dissolve in water by ________ with water, not by releasing S^2- ions into water.