Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO2) and 0.205 M in formic acid (HCO2H). The Ka of formic acid is 1.77 × 10- 4.

A) 4.963 B) 13.84 C) 10.10 D) 3.903 E) 3.587 A) 4.963 B) 13.84 C) 10.10 D) 3.903 E) 3.587

Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid (HCO2H) and 0.230 mol of sodium formate (NaCO2H) in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10- 4.

A) 3.54 B) 10.46 C) 2.09 D) 3.95 E) 2.30 A) 3.54 B) 10.46 C) 2.09 D) 3.95 E) 2.30

Consider the following table of KS1U1B1sp S1U1B0values. -Which compound listed below has the greatest molar solubility in water?

A) CdCO3 B) AgI C) ZnCO3 D) CaF2 E) Cd(OH)2 A) CdCO3 B) AgI C) ZnCO3 D) CaF2 E) Cd(OH)2

What is the molar solubility of barium fluoride ( BaF2 ) in water? The solubility- product constant for BaF2 is 1.7 × 10- 6 at 25°C.

A) 1.2 × 10- 2 B) 1.8 × 10- 3 C) 5.7 × 10- 7 D) 6.5 × 10- 4 E) 7.5 × 10- 3 A) 1.2 × 10- 2 B) 1.8 × 10- 3 C) 5.7 × 10- 7 D) 6.5 × 10- 4 E) 7.5 × 10- 3

The Ksp for Zn(OH)2 is 5.0 × 10- 17. Determine the molar solubility of Zn(OH)2 in a buffer solution with a pH of 11.5.

A) 1.2 × 10- 12 B) 5.0 × 10- 12 C) 1.6 × 10- 14 D) 5.0 × 10- 17 E) 5.0 × 106 A) 1.2 × 10- 12 B) 5.0 × 10- 12 C) 1.6 × 10- 14 D) 5.0 × 10- 17 E) 5.0 × 106

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.219 M in formic acid. The Ka of formic acid is 1.77 × 10- 4.

A) 12.2 B) 3.94 × 10- 5 C) 0.280 D) 0.0180 E) 2.87 A) 12.2 B) 3.94 × 10- 5 C) 0.280 D) 0.0180 E) 2.87

The solubility of manganese (II) hydroxide (Mn(OH)2) is 2.2 × 10- 5 M. What is the Ksp of Mn (OH)2?

A) 4.8 × 10- 10 B) 2.2 × 10- 5 C) 2.1 × 10- 14 D) 4.3 × 10- 14 E) 1.1 × 10- 14 A) 4.8 × 10- 10 B) 2.2 × 10- 5 C) 2.1 × 10- 14 D) 4.3 × 10- 14 E) 1.1 × 10- 14

The solubility of lead (II) chloride (PbCl2) is 1.6 × 10-2 M. What is the Ksp of PbCl2?

A) 1.6 × 10- 5 B) 5.0 × 10- 4 C) 1.6 × 10- 2 D) 4.1 × 10- 6 E) 3.1 × 10- 7 A) 1.6 × 10- 5 B) 5.0 × 10- 4 C) 1.6 × 10- 2 D) 4.1 × 10- 6 E) 3.1 × 10- 7

In which aqueous system is PbI2 least soluble?

A) 0.5 M HI B) 1.0 M HNO3 C) 0.2 M HI D) 0.8 M KI E) H2O A) 0.5 M HI B) 1.0 M HNO3 C) 0.2 M HI D) 0.8 M KI E) H2O

Exam 17: Additional Aspects of Equilibria

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 5.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __ M.

(Multiple Choice)

4.8/5

(35)

Question 21

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10^-⁵.

(Short Answer)

4.8/5

(33)

Question 22

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO₂) and 0.205 M in formic acid (HCO₂H). The K_aof formic acid is 1.77 × 10^-⁴.

(Multiple Choice)

4.8/5

(33)

Question 23

Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid (HCO₂H) and 0.230 mol of sodium formate (NaCO₂H) in water sufficient to yield 1.00 L of solution. The K_aof formic acid is 1.77 × 10^-⁴.

(Multiple Choice)

4.7/5

(36)

Question 24

Consider the following table of K_spvalues. -Which compound listed below has the greatest molar solubility in water?

(Multiple Choice)

4.9/5

(30)

Question 25

A 25.0 mL sample of 0.723 M HClO₄is titrated with a 0.273 M KOH solution. What is the [H⁺] (molarity) before any base is added?

(Multiple Choice)

4.9/5

(45)

Question 26

Which of the following could be added to a solution of sodium acetate to produce a buffer? acetic acid hydrochloric acid potassium acetate sodium chloride

(Multiple Choice)

4.9/5

(37)

Question 27

Which one of the following will cause hemoglobin to release oxygen?

(Multiple Choice)

4.9/5

(43)

Question 28

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. Which of the following indicators would be best for this titration?

(Multiple Choice)

5.0/5

(30)

Question 29

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after addition of 5.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __ M.

(Multiple Choice)

4.8/5

(32)

Question 30

What is the molar solubility of barium fluoride ( BaF₂) in water? The solubility- product constant for BaF₂is 1.7 × 10^-⁶at 25°C.

(Multiple Choice)

4.7/5

(36)

Question 31

The concentration of iodide ions in a saturated solution of lead (II) iodide is M. The solubility product constant of PbI₂is 1.4 × 10^-⁸.

(Multiple Choice)

4.9/5

(32)

Question 32

The K_spfor Zn(OH)₂is 5.0 × 10^-¹⁷. Determine the molar solubility of Zn(OH)₂in a buffer solution with a pH of 11.5.

(Multiple Choice)

4.7/5

(34)

Question 33

Calculate the percent ionization of formic acid (HCO₂H) in a solution that is 0.219 M in formic acid. The K_aof formic acid is 1.77 × 10^-⁴.

(Multiple Choice)

4.8/5

(29)

Question 34

For which salt should the aqueous solubility be most sensitive to pH?

(Multiple Choice)

4.9/5

(37)

Question 35

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The K_aof hypochlorous acid is 3.0 × 10^-⁸.

(Multiple Choice)

4.7/5

(45)

Question 36

The solubility of manganese (II) hydroxide (Mn(OH)₂) is 2.2 × 10^-⁵M. What is the Ksp of Mn (OH)₂?

(Multiple Choice)

4.8/5

(32)

Question 37

The solubility of lead (II) chloride (PbCl₂) is 1.6 × 10^-2 M. What is the Ksp of PbCl₂?

(Multiple Choice)

4.9/5

(32)

Question 38

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

(True/False)

4.8/5

(44)

Question 39

In which aqueous system is PbI₂least soluble?

(Multiple Choice)

4.8/5

(36)

Question 40

Showing 21 - 40 of 88

Exam 17: Additional Aspects of Equilibria

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 5.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __ M.

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10- 5.

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO2) and 0.205 M in formic acid (HCO2H). The Ka of formic acid is 1.77 × 10- 4.

Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid (HCO2H) and 0.230 mol of sodium formate (NaCO2H) in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10- 4.

Consider the following table of Ksp values. -Which compound listed below has the greatest molar solubility in water?

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. What is the [H+] (molarity) before any base is added?

Which of the following could be added to a solution of sodium acetate to produce a buffer? acetic acid hydrochloric acid potassium acetate sodium chloride

Which one of the following will cause hemoglobin to release oxygen?

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. Which of the following indicators would be best for this titration?

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after addition of 5.00 mL of 0.0100 M HCl to 25.0 mL of this solution is __ M.

What is the molar solubility of barium fluoride ( BaF2 ) in water? The solubility- product constant for BaF2 is 1.7 × 10- 6 at 25°C.

The concentration of iodide ions in a saturated solution of lead (II) iodide is M. The solubility product constant of PbI2 is 1.4 × 10- 8.

The Ksp for Zn(OH)2 is 5.0 × 10- 17. Determine the molar solubility of Zn(OH)2 in a buffer solution with a pH of 11.5.

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.219 M in formic acid. The Ka of formic acid is 1.77 × 10- 4.

For which salt should the aqueous solubility be most sensitive to pH?

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The Ka of hypochlorous acid is 3.0 × 10- 8.

The solubility of manganese (II) hydroxide (Mn(OH)2) is 2.2 × 10- 5 M. What is the Ksp of Mn (OH)2?

The solubility of lead (II) chloride (PbCl2) is 1.6 × 10-2 M. What is the Ksp of PbCl2?

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

In which aqueous system is PbI2 least soluble?

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

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.770× 10^-⁵.

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO₂) and 0.205 M in formic acid (HCO₂H). The K_aof formic acid is 1.77 × 10^-⁴.

Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid (HCO₂H) and 0.230 mol of sodium formate (NaCO₂H) in water sufficient to yield 1.00 L of solution. The K_aof formic acid is 1.77 × 10^-⁴.

Consider the following table of K_spvalues. -Which compound listed below has the greatest molar solubility in water?

A 25.0 mL sample of 0.723 M HClO₄is titrated with a 0.273 M KOH solution. What is the [H⁺] (molarity) before any base is added?

What is the molar solubility of barium fluoride ( BaF₂) in water? The solubility- product constant for BaF₂is 1.7 × 10^-⁶at 25°C.

The concentration of iodide ions in a saturated solution of lead (II) iodide is M. The solubility product constant of PbI₂is 1.4 × 10^-⁸.

The K_spfor Zn(OH)₂is 5.0 × 10^-¹⁷. Determine the molar solubility of Zn(OH)₂in a buffer solution with a pH of 11.5.

Calculate the percent ionization of formic acid (HCO₂H) in a solution that is 0.219 M in formic acid. The K_aof formic acid is 1.77 × 10^-⁴.

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The K_aof hypochlorous acid is 3.0 × 10^-⁸.

The solubility of manganese (II) hydroxide (Mn(OH)₂) is 2.2 × 10^-⁵M. What is the Ksp of Mn (OH)₂?

The solubility of lead (II) chloride (PbCl₂) is 1.6 × 10^-2 M. What is the Ksp of PbCl₂?

In which aqueous system is PbI₂least soluble?