Question 1

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.

Accepted Answer

A)  0.00167 
B)  0.00253 
C)  0.0817 
D)  0.0980 
E)  0.0850

Question 2

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.

Accepted Answer

The answer of Suppose you have just added 100.0 ml...

Question 3

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.

Accepted Answer

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

Question 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.

Accepted Answer

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

Question 5

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

Accepted Answer

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

Question 6

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?

Accepted Answer

A)  0.439 
B)  1.00 × 10- 7 
C)  0.723 
D)  0.273 
E)  2.81 × 10- 13

Question 7

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

Accepted Answer

A)  sodium chloride or potassium acetate 
B)  potassium acetate only 
C)  hydrochloric acid only 
D)  acetic acid or hydrochloric acid 
E)  acetic acid only

Question 8

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

Accepted Answer

A)  decrease in pH 
B)  increase in pH 
C)  increase in O2 concentration 
D)  decrease in temperature 
E)  decrease in CO2 concentration

Question 9

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?

Accepted Answer

A)  thymol blue 
B)  bromthymol blue 
C)  phenolpthalein 
D)  bromocresol purple 
E)  methyl red

Question 10

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.

Accepted Answer

A)  0.00976 
B)  0.00193 
C)  0.100 
D)  0.126 
E)  0.107

Question 11

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.

Accepted Answer

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

Question 12

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.

Accepted Answer

A)  3.8 × 10- 4  
B)  3.5 × 10- 9  
C)  1.5 × 10- 3  
D)  1.4 × 10- 8  
E)  3.0 × 10- 3

Question 13

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.

Accepted Answer

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

Question 14

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.

Accepted Answer

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

Question 15

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

Accepted Answer

A)  CaF2  
B)  CaCl2  
C)  Ca(NO3)2  
D)  CaBr2  
E)  CaI2

Question 16

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.

Accepted Answer

A)  11.47 
B)  2.54 
C)  7.54 
D)  7.51 
E)  7.00

Question 17

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

Accepted Answer

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

Question 18

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

Accepted Answer

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

Question 19

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.

Accepted Answer

A) True 
 B)False

Question 20

In which aqueous system is PbI2 least soluble?

Accepted Answer

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.

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?

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 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.

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 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?

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 PbI₂least soluble?

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?

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?