Calculate the pH of a solution prepared by dissolving 0.750 mol of NH3 and 0.250 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10- 4.

A) 8.78 B) 0.89 C) 9.73 D) 4.27 E) 5.22 A) 8.78 B) 0.89 C) 9.73 D) 4.27 E) 5.22 C

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10- 6.

A) 1.1 × 10- 2 B) 1.2 × 10- 4 C) 2.4 × 10- 8 D) 2.7 × 10- 3 E) 5.9 × 10- 5 A) 1.1 × 10- 2 B) 1.2 × 10- 4 C) 2.4 × 10- 8 D) 2.7 × 10- 3 E) 5.9 × 10- 5

A) slightly acidic B) slightly basic C) very basic D) very acidic E) neutral A) slightly acidic B) slightly basic C) very basic D) very acidic E) neutral

Exam 17: Additional Aspects of Equilibria

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is M.

Free

(Multiple Choice)

4.8/5

(35)

Question 1

Correct Answer:

Verified

Calculate the pH of a solution prepared by dissolving 0.750 mol of NH₃and 0.250 mol of NH₄Cl in water sufficient to yield 1.00 L of solution. The K_bof ammonia is 1.77 × 10^-⁴.

Free

(Multiple Choice)

4.9/5

(34)

Question 2

Correct Answer:

Verified

Which below best describe(s) the behavior of an amphoteric hydroxide in water?

Free

(Multiple Choice)

4.8/5

(40)

Question 3

Correct Answer:

Verified

A 50.0 mL sample of an aqueous H₂SO₄solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H₂SO₄is _ _ M.

(Multiple Choice)

4.8/5

(47)

Question 4

In which of the following aqueous solutions would you expect AgBr to have the highest solubility?

(Multiple Choice)

4.9/5

(35)

Question 5

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

(True/False)

4.9/5

(31)

Question 6

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba²⁺. When the concentration of F^-exceeds M, BaF₂will precipitate. Neglect volume changes. For BaF₂, K_sp= 1.7 × 10^-⁶.

(Multiple Choice)

4.9/5

(33)

Question 7

Human blood is .

(Multiple Choice)

4.8/5

(32)

Question 8

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid (HBz) and 0)300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The K_aof benzoic acid is 6.50 × 10^-⁵.

(Multiple Choice)

4.9/5

(40)

Question 9

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10^-⁴.

(Short Answer)

4.9/5

(35)

Question 10

Which one of the following pairs cannot be mixed together to form a buffer solution?

(Multiple Choice)

4.7/5

(34)

Question 11

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The K_aof nitrous acid is 4.50 × 10^-⁴.

(Multiple Choice)

4.9/5

(34)

Question 12

Of the following solutions, which has the greatest buffering capacity?

(Multiple Choice)

4.7/5

(33)

Question 13

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

(Multiple Choice)

4.9/5

(44)

Question 14

The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is )

(Multiple Choice)

4.8/5

(41)

Question 15

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about mol/L.

(Multiple Choice)

4.8/5

(38)

Question 16

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?

(Multiple Choice)

4.7/5

(42)

Question 17

The molar solubility of _ is not affected by the pH of the solution.

(Multiple Choice)

4.8/5

(29)

Question 18

Which of the following could be added to a solution of potassium fluoride to prepare a buffer?

(Multiple Choice)

4.8/5

(33)

Question 19

Which of the following could be added to a solution of acetic acid to prepare a buffer? sodium acetate sodium hydroxide nitric acid hydrofluoric acid

(Multiple Choice)

5.0/5

(25)

Question 20

Showing 1 - 20 of 88

Exam 17: Additional Aspects of Equilibria

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is M.

Calculate the pH of a solution prepared by dissolving 0.750 mol of NH3 and 0.250 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10- 4.

Which below best describe(s) the behavior of an amphoteric hydroxide in water?

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is _ _ M.

In which of the following aqueous solutions would you expect AgBr to have the highest solubility?

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10- 6.

Human blood is .

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid (HBz) and 0)300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10- 5.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10- 4.

Which one of the following pairs cannot be mixed together to form a buffer solution?

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of nitrous acid is 4.50 × 10- 4.

Of the following solutions, which has the greatest buffering capacity?

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

The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is )

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about mol/L.

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?

The molar solubility of _ is not affected by the pH of the solution.

Which of the following could be added to a solution of potassium fluoride to prepare a buffer?

Which of the following could be added to a solution of acetic acid to prepare a buffer? sodium acetate sodium hydroxide nitric acid hydrofluoric acid

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

Filters

Calculate the pH of a solution prepared by dissolving 0.750 mol of NH₃and 0.250 mol of NH₄Cl in water sufficient to yield 1.00 L of solution. The K_bof ammonia is 1.77 × 10^-⁴.

A 50.0 mL sample of an aqueous H₂SO₄solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H₂SO₄is _ _ M.

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba²⁺. When the concentration of F^-exceeds M, BaF₂will precipitate. Neglect volume changes. For BaF₂, K_sp= 1.7 × 10^-⁶.

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid (HBz) and 0)300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The K_aof benzoic acid is 6.50 × 10^-⁵.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10^-⁴.

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The K_aof nitrous acid is 4.50 × 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 before any base is added? The K_aof butanoic acid is 1.5 × 10^-⁵.