Solid potassium chromate (K2CrO4)is slowly added to a solution containing 0.50 mol L-1 AgNO3 and 0.50 mol L-1 Ba(NO3)2.What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and $1.2 \times 10 ^{- 10} \text {, }$ respectively.

A) 6.5 × 10-5 mol L-1 B) 1.3 × 10-4 mol L-1 C) 3.2 × 10-4 mol L-1 D) 6.8 × 10-2 mol L-1 A) 6.5 × 10-5 mol L-1 B) 1.3 × 10-4 mol L-1 C) 3.2 × 10-4 mol L-1 D) 6.8 × 10-2 mol L-1

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 mol L-1 CH3COOH with 25.00 mL of 0.010 mol L-1 CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3COOH.

A) 2.87 B) 3.74 C) 4.75 D) 5.74 A) 2.87 B) 3.74 C) 4.75 D) 5.74

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 HNO3.Determine the pH of the solution after the addition of 150.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

A) 1.7 B) 6.4 C) 7.6 D) 12.3 E) 2.3 A) 1.7 B) 6.4 C) 7.6 D) 12.3 E) 2.3

You wish to prepare a buffer containing CH3COOH with a pH of 5.44.If the pKa of acetic acid is 4.74,what ratio of [CH3COO-]/[CH3COOH] must you use?

A) 0.70 B) 0.20 C) 1.4 D) 5.0 E) 1.1 A) 0.70 B) 0.20 C) 1.4 D) 5.0 E) 1.1

Determine the molar solubility of CaSO4 in a solution containing 0.100 mol L-1 Na2SO4.Ksp (CaSO4)= 2.4 × 10-5.

A) 4.9 × 10-3 mol L-1 B) 2.4 × 10-4 mol L-1 C) 5.8 × 10-10 mol L-1 D) 1.2 × 10-5 mol L-1 E) 0.10 mol L-1 A) 4.9 × 10-3 mol L-1 B) 2.4 × 10-4 mol L-1 C) 5.8 × 10-10 mol L-1 D) 1.2 × 10-5 mol L-1 E) 0.10 mol L-1

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.50? Ksp for Mg(OH)2 is $5.6 \times 10 ^{- 12}$

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

Determine the molar solubility of BaF2 in a solution containing 0.0750 mol L-1 LiF.Ksp (BaF2)= 1.7 × 10-6.

A) 2.3 × 10-5 mol L-1 B) 8.5 × 10-7 mol L-1 C) 1.2 × 10-2 mol L-1 D) 0.075 mol L-1 E) 3.0 × 10-4 mol L-1 A) 2.3 × 10-5 mol L-1 B) 8.5 × 10-7 mol L-1 C) 1.2 × 10-2 mol L-1 D) 0.075 mol L-1 E) 3.0 × 10-4 mol L-1

Exam 16: Aqueous Ionic Equilibrium

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH.Determine the pH of the solution before the addition of any KOH.The K_a of HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 21

Calculate the pH of a buffer that is 0.058 mol L^-1 HF and 0.058 mol L^-1 LiF.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 22

Identify the expression for the solubility product constant for BaF₂.

(Multiple Choice)

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Question 23

What happens at low pH to aluminum hydroxide precipitate?

(Multiple Choice)

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Question 24

Identify the indicator that has two endpoints.

(Multiple Choice)

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Question 25

Which of the following is the correct equation relating Q to K_sp for a saturated solution?

(Multiple Choice)

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Question 26

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L^-1 HCl to reach the equivalence point?

(Multiple Choice)

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Question 27

Solid potassium chromate (K₂CrO₄)is slowly added to a solution containing 0.50 mol L^-1 AgNO₃ and 0.50 mol L^-1 Ba(NO₃)₂.What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and $1.2 \times 10 ^{- 10} \text {, }$ respectively.

(Multiple Choice)

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Question 28

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 mol L^-1 CH₃COOH with 25.00 mL of 0.010 mol L^-1 CH₃COONa? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃COOH.

(Multiple Choice)

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Question 29

A 100.0 mL sample of 0.180 mol L^-1 HClO₄ is titrated with 0.270 mol L^-1 NaOH.Determine the pH of the solution after the addition of 75.0 mL of NaOH.

(Multiple Choice)

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Question 30

What is the pH of a buffer solution that is 0.251 mol L^-1 in lactic acid and 0.151 mol L^-1 in sodium lactate? The $K _ { a }$ of lactic acid is 1.4 × $10 ^ { - 4 }$ .

(Multiple Choice)

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Question 31

A 100.0 mL sample of 0.10 mol L^-1 NH₃ is titrated with 0.10 mol L^-1 HNO₃.Determine the pH of the solution after the addition of 150.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

(Multiple Choice)

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Question 32

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of a 0.12 mol L^-1 LiOH solution.What is the concentration of the H₂SO₄ solution (in mol L^-1)?

(Multiple Choice)

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Question 33

Identify a good buffer.

(Multiple Choice)

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Question 34

You wish to prepare a buffer containing CH₃COOH with a pH of 5.44.If the pK_a of acetic acid is 4.74,what ratio of [CH₃COO^-]/[CH₃COOH] must you use?

(Multiple Choice)

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Question 35

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L^-1 HClO with 300.0 mL of 0.20 mol L^-1 KClO.The K_a for HClO is 2.9 × 10^-8.

(Multiple Choice)

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Question 36

Determine the molar solubility of CaSO₄ in a solution containing 0.100 mol L^-1 Na₂SO₄.K_sp (CaSO₄)= 2.4 × 10^-5.

(Multiple Choice)

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Question 37

If the pK_a of HCOOH is 3.74 and the pH of an HCOOH/HCOONabuffer solution is 3.74,which of the following is TRUE?

(Multiple Choice)

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Question 38

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is $5.6 \times 10 ^{- 12}$

(Multiple Choice)

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Question 39

Determine the molar solubility of BaF₂ in a solution containing 0.0750 mol L^-1 LiF.K_sp (BaF₂)= 1.7 × 10^-6.

(Multiple Choice)

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Question 40

Showing 21 - 40 of 159

Exam 16: Aqueous Ionic Equilibrium

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH.Determine the pH of the solution before the addition of any KOH.The Ka of HF is 3.5 × 10-4.

Calculate the pH of a buffer that is 0.058 mol L-1 HF and 0.058 mol L-1 LiF.The Ka for HF is 3.5 × 10-4.

Identify the expression for the solubility product constant for BaF2.

What happens at low pH to aluminum hydroxide precipitate?

Identify the indicator that has two endpoints.

Which of the following is the correct equation relating Q to Ksp for a saturated solution?

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L-1 HCl to reach the equivalence point?

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 mol L-1 CH3COOH with 25.00 mL of 0.010 mol L-1 CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3COOH.

A 100.0 mL sample of 0.180 mol L-1 HClO4 is titrated with 0.270 mol L-1 NaOH.Determine the pH of the solution after the addition of 75.0 mL of NaOH.

What is the pH of a buffer solution that is 0.251 mol L-1 in lactic acid and 0.151 mol L-1 in sodium lactate? The KaK _ { a }Ka​ of lactic acid is 1.4 × 10−410 ^ { - 4 }10−4 .

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 HNO3.Determine the pH of the solution after the addition of 150.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of a 0.12 mol L-1 LiOH solution.What is the concentration of the H2SO4 solution (in mol L-1)?

Identify a good buffer.

You wish to prepare a buffer containing CH3COOH with a pH of 5.44.If the pKa of acetic acid is 4.74,what ratio of [CH3COO-]/[CH3COOH] must you use?

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L-1 HClO with 300.0 mL of 0.20 mol L-1 KClO.The Ka for HClO is 2.9 × 10-8.

Determine the molar solubility of CaSO4 in a solution containing 0.100 mol L-1 Na2SO4.Ksp (CaSO4)= 2.4 × 10-5.

If the pKa of HCOOH is 3.74 and the pH of an HCOOH/HCOONa buffer solution is 3.74,which of the following is TRUE?

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.50? Ksp for Mg(OH)2 is 5.6×10−125.6 \times 10 ^{- 12}5.6×10−12

Determine the molar solubility of BaF2 in a solution containing 0.0750 mol L-1 LiF.Ksp (BaF2)= 1.7 × 10-6.

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A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH.Determine the pH of the solution before the addition of any KOH.The K_a of HF is 3.5 × 10^-4.

Calculate the pH of a buffer that is 0.058 mol L^-1 HF and 0.058 mol L^-1 LiF.The K_a for HF is 3.5 × 10^-4.

Identify the expression for the solubility product constant for BaF₂.

Which of the following is the correct equation relating Q to K_sp for a saturated solution?

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L^-1 HCl to reach the equivalence point?

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 mol L^-1 CH₃COOH with 25.00 mL of 0.010 mol L^-1 CH₃COONa? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃COOH.

A 100.0 mL sample of 0.180 mol L^-1 HClO₄ is titrated with 0.270 mol L^-1 NaOH.Determine the pH of the solution after the addition of 75.0 mL of NaOH.

What is the pH of a buffer solution that is 0.251 mol L^-1 in lactic acid and 0.151 mol L^-1 in sodium lactate? The $K _ { a }$ of lactic acid is 1.4 × $10 ^ { - 4 }$ .

A 100.0 mL sample of 0.10 mol L^-1 NH₃ is titrated with 0.10 mol L^-1 HNO₃.Determine the pH of the solution after the addition of 150.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of a 0.12 mol L^-1 LiOH solution.What is the concentration of the H₂SO₄ solution (in mol L^-1)?

You wish to prepare a buffer containing CH₃COOH with a pH of 5.44.If the pK_a of acetic acid is 4.74,what ratio of [CH₃COO^-]/[CH₃COOH] must you use?

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L^-1 HClO with 300.0 mL of 0.20 mol L^-1 KClO.The K_a for HClO is 2.9 × 10^-8.

Determine the molar solubility of CaSO₄ in a solution containing 0.100 mol L^-1 Na₂SO₄.K_sp (CaSO₄)= 2.4 × 10^-5.

If the pK_a of HCOOH is 3.74 and the pH of an HCOOH/HCOONabuffer solution is 3.74,which of the following is TRUE?

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is $5.6 \times 10 ^{- 12}$

Determine the molar solubility of BaF₂ in a solution containing 0.0750 mol L^-1 LiF.K_sp (BaF₂)= 1.7 × 10^-6.