In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25 °C?

A) 0.1 mol L-1 HBr B) 0.1 mol L-1 NaBr C) 0.1 mol L-1 CaBr2 D) 0.1 mol L-1 K NO3 A) 0.1 mol L-1 HBr B) 0.1 mol L-1 NaBr C) 0.1 mol L-1 CaBr2 D) 0.1 mol L-1 K NO3 C

Calculate the pH of a buffer that is 0.225 mol L-1 CH3COOH and 0.162 mol L-1 CH3COOK. The Ka for CH3COOH is 1.8 × 10-5.

A) 4.89 B) 9.11 C) 4.74 D) 9.26 E) 4.60 A) 4.89 B) 9.11 C) 4.74 D) 9.26 E) 4.60

A 1.0 L buffer solution is 0.250 mol L-1 CH3COOH and 0.050 mol L-1 CH3COOLi. Which of the following actions will exceed the capacity of the buffer?

A) adding 0.050 moles of CH3COOLi B) adding 0.050 moles of CH3COOH C) adding 0.050 moles of HCl D) adding 0.050 moles of NaCl E) adding 0.050 moles of NH4Cl A) adding 0.050 moles of CH3COOLi B) adding 0.050 moles of CH3COOH C) adding 0.050 moles of HCl D) adding 0.050 moles of NaCl E) adding 0.050 moles of NH4Cl

A 1.0 L buffer solution is 0.050 mol L-1 CH3COOH and 0.250 mol L-1 CH3COOLi. Which of the following actions will destroy the buffer?

A) adding 0.050 moles of NaOH B) adding 0.050 moles of HCl C) adding 0.050 moles of CH3COOH D) adding 0.050 moles of CH3COOLi E) adding 0.050 moles of NH4Cl. A) adding 0.050 moles of NaOH B) adding 0.050 moles of HCl C) adding 0.050 moles of CH3COOH D) adding 0.050 moles of CH3COOLi E) adding 0.050 moles of NH4Cl.

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate formed upon the addition of 6 mol L-1 HCl.

A) Ba3(PO4)2 B) CdS C) AgCl D) NH4Cl E) ZnS A) Ba3(PO4)2 B) CdS C) AgCl D) NH4Cl E) ZnS

Determine the molar solubility of PbSO4 in pure water. Ksp (PbSO4)= 1.82 × 10-8.

A) 1.82 × 10-8 mol L-1 B) 1.35 × 10-4 mol L-1 C) 9.10 × 10-9 mol L-1 D) 3.31 × 10-16 mol L-1 E) 4.48 × 10-4 mol L-1 A) 1.82 × 10-8 mol L-1 B) 1.35 × 10-4 mol L-1 C) 9.10 × 10-9 mol L-1 D) 3.31 × 10-16 mol L-1 E) 4.48 × 10-4 mol L-1

Determine the molar solubility of Fe(OH)2 in pure water. Ksp for Fe(OH)2 = 4.87 × 10-17.

A) 2.44 × 10-17 mol L-1 B) 1.62 × 10-17 mol L-1 C) 4.03 × 10-9 mol L-1 D) 3.65 × 10-6 mol L-1 E) 2.30 × 10-6 mol L-1 A) 2.44 × 10-17 mol L-1 B) 1.62 × 10-17 mol L-1 C) 4.03 × 10-9 mol L-1 D) 3.65 × 10-6 mol L-1 E) 2.30 × 10-6 mol L-1

Exam 16: Aqueous Ionic Equilibrium

Calculate the percent ionization of nitrous acid in a solution that is 0.249 mol L^-1 in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Free

(Multiple Choice)

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Question 1

Correct Answer:

Verified

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C?

Free

(Multiple Choice)

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Question 2

Correct Answer:

Verified

The molar solubility of CuI is 2.26 × 10^-6 mol L^-1 in pure water. Calculate the K_sp for CuI.

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH. Determine the pH of the solution after the addition of 100.0 mL of NaOH.

(Multiple Choice)

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Question 4

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L^-1 acetic acid with 10.00 mL of 0.10 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for CH₃COOH.

(Multiple Choice)

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Question 5

Calculate the pH of a buffer that is 0.225 mol L^-1 CH₃COOH and 0.162 mol L^-1 CH₃COOK. The K_a for CH₃COOH is 1.8 × 10^-5.

(Multiple Choice)

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Question 6

A 1.0 L buffer solution is 0.250 mol L^-1 CH₃COOH and 0.050 mol L^-1 CH₃COOLi. Which of the following actions will exceed the capacity of the buffer?

(Multiple Choice)

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Question 7

Identify the expression for the solubility product constant for Cr₂(CO₃)₃.

(Multiple Choice)

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Question 8

Identify the expression for the solubility product constant for BaF₂.

(Multiple Choice)

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Question 9

Give the name of the compound that is in antifreeze and is toxic to pets.

(Short Answer)

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Question 10

Which of the following compounds will have the highest molar solubility in pure water?

(Multiple Choice)

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Question 11

Identify the salts that are in hard water.

(Multiple Choice)

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Question 12

A 1.0 L buffer solution is 0.050 mol L^-1 CH₃COOH and 0.250 mol L^-1 CH₃COOLi. Which of the following actions will destroy the buffer?

(Multiple Choice)

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Question 13

Identify a good buffer.

(Multiple Choice)

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Question 14

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 15

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate formed upon the addition of 6 mol L^-1 HCl.

(Multiple Choice)

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Question 16

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH. Determine the pH of the solution after the addition of 66.67 mL of NaOH (this is the equivalence point).

(Multiple Choice)

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Question 17

Determine the molar solubility of PbSO₄ in pure water. K_sp (PbSO₄)= 1.82 × 10^-8.

(Multiple Choice)

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Question 18

Determine the molar solubility of Fe(OH)₂in pure water. K_sp for Fe(OH)₂ = 4.87 × 10^-17.

(Multiple Choice)

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Question 19

A 1.00 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in LiF. Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of the base. The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 20

Showing 1 - 20 of 161

Exam 16: Aqueous Ionic Equilibrium

Calculate the percent ionization of nitrous acid in a solution that is 0.249 mol L-1 in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10-4.

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25 °C?

The molar solubility of CuI is 2.26 × 10-6 mol L-1 in pure water. Calculate the Ksp for CuI.

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH. Determine the pH of the solution after the addition of 100.0 mL of NaOH.

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L-1 acetic acid with 10.00 mL of 0.10 mol L-1 KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for CH3COOH.

Calculate the pH of a buffer that is 0.225 mol L-1 CH3COOH and 0.162 mol L-1 CH3COOK. The Ka for CH3COOH is 1.8 × 10-5.

A 1.0 L buffer solution is 0.250 mol L-1 CH3COOH and 0.050 mol L-1 CH3COOLi. Which of the following actions will exceed the capacity of the buffer?

Identify the expression for the solubility product constant for Cr2(CO3)3.

Identify the expression for the solubility product constant for BaF2.

Give the name of the compound that is in antifreeze and is toxic to pets.

Which of the following compounds will have the highest molar solubility in pure water?

Identify the salts that are in hard water.

A 1.0 L buffer solution is 0.050 mol L-1 CH3COOH and 0.250 mol L-1 CH3COOLi. Which of the following actions will destroy the buffer?

Identify a good buffer.

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.

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate formed upon the addition of 6 mol L-1 HCl.

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH. Determine the pH of the solution after the addition of 66.67 mL of NaOH (this is the equivalence point).

Determine the molar solubility of PbSO4 in pure water. Ksp (PbSO4)= 1.82 × 10-8.

Determine the molar solubility of Fe(OH)2 in pure water. Ksp for Fe(OH)2 = 4.87 × 10-17.

A 1.00 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in LiF. Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of the base. The Ka for HF is 3.5 × 10-4.

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Calculate the percent ionization of nitrous acid in a solution that is 0.249 mol L^-1 in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C?

The molar solubility of CuI is 2.26 × 10^-6 mol L^-1 in pure water. Calculate the K_sp for CuI.

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH. Determine the pH of the solution after the addition of 100.0 mL of NaOH.

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L^-1 acetic acid with 10.00 mL of 0.10 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for CH₃COOH.

Calculate the pH of a buffer that is 0.225 mol L^-1 CH₃COOH and 0.162 mol L^-1 CH₃COOK. The K_a for CH₃COOH is 1.8 × 10^-5.

A 1.0 L buffer solution is 0.250 mol L^-1 CH₃COOH and 0.050 mol L^-1 CH₃COOLi. Which of the following actions will exceed the capacity of the buffer?

Identify the expression for the solubility product constant for Cr₂(CO₃)₃.

Identify the expression for the solubility product constant for BaF₂.

A 1.0 L buffer solution is 0.050 mol L^-1 CH₃COOH and 0.250 mol L^-1 CH₃COOLi. Which of the following actions will destroy the buffer?

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.

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate formed upon the addition of 6 mol L^-1 HCl.

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH. Determine the pH of the solution after the addition of 66.67 mL of NaOH (this is the equivalence point).

Determine the molar solubility of PbSO₄ in pure water. K_sp (PbSO₄)= 1.82 × 10^-8.

Determine the molar solubility of Fe(OH)₂in pure water. K_sp for Fe(OH)₂ = 4.87 × 10^-17.

A 1.00 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in LiF. Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of the base. The K_a for HF is 3.5 × 10^-4.