Determine the molar solubility of CaSO4 in a solution containing 0.12 M K2SO4. Ksp (CaSO4)= 2.4 × 10-5.

A) 2.9 × 10-6 M B) 2.0 × 10-4 M C) 5.8 × 10-10 M D) 4.9 × 10-3 M E) 0.20 M A) 2.9 × 10-6 M B) 2.0 × 10-4 M C) 5.8 × 10-10 M D) 4.9 × 10-3 M E) 0.20 M

Give the expression for Kf for Co(SCN)42-.

A) B) C) D) [Co4+] [SCN-]4 E) A) B) C) D) [Co4+] [SCN-]4 E)

100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution before the addition of any HNO3.The Kb of NH3 is 1.8 × 10-5.

A) 4.74 B) 9.26 C) 11.13 D) 13.00 E) 12.55 A) 4.74 B) 9.26 C) 11.13 D) 13.00 E) 12.55

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl.What will happen once these solutions are mixed? Ksp (AgCl)= 1.77 × 10-10.

A) Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. B) Silver chloride will precipitate out of solution, leaving an unsaturated solution of AgCl. C) Silver chloride will precipitate out of solution, leaving a saturated AgCl solution. D) Nothing will happen since NaCl and AgNO3 are both soluble compounds. E) There is not enough information to say anything about this solution. A) Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. B) Silver chloride will precipitate out of solution, leaving an unsaturated solution of AgCl. C) Silver chloride will precipitate out of solution, leaving a saturated AgCl solution. D) Nothing will happen since NaCl and AgNO3 are both soluble compounds. E) There is not enough information to say anything about this solution.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 200.0 mL of 0.12 M NH3.The Kb for NH3 is 1.8 × 10-5.

A) 9.06 B) 9.45 C) 4.55 D) 4.74 E) 9.26 A) 9.06 B) 9.45 C) 4.55 D) 4.74 E) 9.26

What is the molar solubility of calcium fluoride (CaF2)in water? The solubility-product constant for CaF2 is 3.9 × 10-11 at 25°C.

A) 3.1 × 10-6 B) 3.4 × 10-4 C) 8.8 × 10-6 D) 2.1 × 10-4 E) 1.3 × 10-11 A) 3.1 × 10-6 B) 3.4 × 10-4 C) 8.8 × 10-6 D) 2.1 × 10-4 E) 1.3 × 10-11

Exam 17: Aqueous Ionic Equilibrium

A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly.The pH does not decrease drastically because the HCl reacts with the __________ present in the buffer solution.The K_a of nitrous acid is 1.36 × 10^-3.

(Multiple Choice)

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Question 81

Determine the molar solubility of CaSO₄ in a solution containing 0.12 M K₂SO₄. K_sp (CaSO₄)= 2.4 × 10^-5.

(Multiple Choice)

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Question 82

Give the expression for K_f for Co(SCN)₄^2-.

(Multiple Choice)

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Question 83

A solution contains 0.036 M Cu²⁺ and 0.044 M Fe²⁺.A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution.At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate? K_sp(CuS)= 1.3 × 10^-36,K_sp(FeS)= 6.3 × 10^-18.

(Multiple Choice)

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Question 84

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 85

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The K_a of butanoic acid is 1.5 × 10^-5.

(Multiple Choice)

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Question 86

100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

(Multiple Choice)

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Question 87

A solution contains 0.021 M Cl⁻ and 0.017 M I⁻.A solution containing copper(I)ions is added to selectively precipitate one of the ions.At what concentration of copper(I)ion will a precipitate begin to form? What is the identity of the precipitate? K_sp(CuCl)= 1.0 × 10^-6,K_sp(CuI)= 5.1 × 10^-12.

(Multiple Choice)

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Question 88

A solution containing AgNO₃ is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO₃ and 0.075 M in NaCl.What will happen once these solutions are mixed? K_sp (AgCl)= 1.77 × 10^-10.

(Multiple Choice)

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Question 89

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.100 moles of solid NaOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 90

The largest change in pH for an effective buffer occurs when the base is how many times as concentrated as the acid?

(Multiple Choice)

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Question 91

Which one of the following statements is TRUE?

(Multiple Choice)

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Question 92

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH after 13.3 mL of base is added? The K_a of butanoic acid is 1.5 × 10^-5.

(Multiple Choice)

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Question 93

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The K_a of lactic acid is 1.4 × 10^-4.

(Multiple Choice)

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Question 94

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH₄Cl with 200.0 mL of 0.12 M NH₃.The K_b for NH₃ is 1.8 × 10^-5.

(Multiple Choice)

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Question 95

What is the molar solubility of calcium fluoride (CaF₂)in water? The solubility-product constant for CaF₂ is 3.9 × 10^-11 at 25°C.

(Multiple Choice)

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Question 96

A complex ion contains

(Multiple Choice)

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Question 97

Calculate the pH of a buffer that is 0.020 M HF and 0.040 M NaF.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 98

Calculate the pH of a buffer that is 0.032 M HF and 0.032 M NaF.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 99

When a diprotic acid is titrated with a strong base,and the K_a1 and K_a2 are significantly different,then the pH vs.volume plot of the titration will have

(Multiple Choice)

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Question 100

Showing 81 - 100 of 187

Exam 17: Aqueous Ionic Equilibrium

Determine the molar solubility of CaSO4 in a solution containing 0.12 M K2SO4. Ksp (CaSO4)= 2.4 × 10-5.

Give the expression for Kf for Co(SCN)42-.

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The Ka of butanoic acid is 1.5 × 10-5.

100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution before the addition of any HNO3.The Kb of NH3 is 1.8 × 10-5.

A solution contains 0.021 M Cl⁻ and 0.017 M I⁻.A solution containing copper(I)ions is added to selectively precipitate one of the ions.At what concentration of copper(I)ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuCl)= 1.0 × 10-6,Ksp(CuI)= 5.1 × 10-12.

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl.What will happen once these solutions are mixed? Ksp (AgCl)= 1.77 × 10-10.

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.100 moles of solid NaOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

The largest change in pH for an effective buffer occurs when the base is how many times as concentrated as the acid?

Which one of the following statements is TRUE?

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH after 13.3 mL of base is added? The Ka of butanoic acid is 1.5 × 10-5.

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 200.0 mL of 0.12 M NH3.The Kb for NH3 is 1.8 × 10-5.

What is the molar solubility of calcium fluoride (CaF2)in water? The solubility-product constant for CaF2 is 3.9 × 10-11 at 25°C.

A complex ion contains

Calculate the pH of a buffer that is 0.020 M HF and 0.040 M NaF.The Ka for HF is 3.5 × 10-4.

Calculate the pH of a buffer that is 0.032 M HF and 0.032 M NaF.The Ka for HF is 3.5 × 10-4.

When a diprotic acid is titrated with a strong base,and the Ka1 and Ka2 are significantly different,then the pH vs.volume plot of the titration will have

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Determine the molar solubility of CaSO₄ in a solution containing 0.12 M K₂SO₄. K_sp (CaSO₄)= 2.4 × 10^-5.

Give the expression for K_f for Co(SCN)₄^2-.

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The K_a of butanoic acid is 1.5 × 10^-5.

100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

A solution containing AgNO₃ is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO₃ and 0.075 M in NaCl.What will happen once these solutions are mixed? K_sp (AgCl)= 1.77 × 10^-10.

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.100 moles of solid NaOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH after 13.3 mL of base is added? The K_a of butanoic acid is 1.5 × 10^-5.

What is the pH of a buffer solution that is 0.211 M in lactic acid and 0.111 M in sodium lactate? The K_a of lactic acid is 1.4 × 10^-4.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH₄Cl with 200.0 mL of 0.12 M NH₃.The K_b for NH₃ is 1.8 × 10^-5.

What is the molar solubility of calcium fluoride (CaF₂)in water? The solubility-product constant for CaF₂ is 3.9 × 10^-11 at 25°C.

Calculate the pH of a buffer that is 0.020 M HF and 0.040 M NaF.The K_a for HF is 3.5 × 10^-4.

Calculate the pH of a buffer that is 0.032 M HF and 0.032 M NaF.The K_a for HF is 3.5 × 10^-4.

When a diprotic acid is titrated with a strong base,and the K_a1 and K_a2 are significantly different,then the pH vs.volume plot of the titration will have