Question 1

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M hypochlorous acid to the equivalence point? The Ka of hypochlorous acid is 3.0 × 10-8.

Accepted Answer

A) 7.60 
B) 50.0 
C) 41.6 
D) 60.1 
E) 7.35

Question 2

A solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium hypochlorite in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution. The Ka of hypochlorous acid is 1.36 × 10-3.

Accepted Answer

A) H2O 
B) H3O+ 
C) hypochlorite ion 
D) hypochlorous acid 
E) This is a buffer solution: the pH does not change upon addition of acid or base.

Question 3

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

Accepted Answer

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

Question 4

The Kb of ammonia is 1.76 × 10-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate is ________.

Accepted Answer

A) 4.632 
B) 9.291 
C) 4.742 
D) 9.372 
E) none of the above

Question 5

The primary buffer system that controls the pH of the blood is the ________ buffer system.

Accepted Answer

A) carbon dioxide, carbonate 
B) carbonate, bicarbonate 
C) carbonic acid, carbon dioxide 
D) carbonate, carbonic acid 
E) carbonic acid, bicarbonate

Question 6

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Accepted Answer

The answer of Suppose you have just added 200.0 ml...

Question 7

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

Accepted Answer

A) 11.20 
B) 9.80 
C) 4.20 
D) 7.00 
E) 8.54

Question 8

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 13.3 mL of base is added? The Ka of hypochlorous acid is 3.0 × 10-8.

Accepted Answer

A) 7.25 
B) 1.34 
C) 4.43 
D) 7.58 
E) 7.46

Question 9

An assembly of a metal ion and the Lewis bases bonded to it is called a(n)________.

Accepted Answer

The answer of An assembly of a metal ion and...

Question 10

The addition of hydrochloric acid and ________ to water produces a buffer solution.

Accepted Answer

A) HC6H5O 
B) NaOH 
C) NH3 
D) HNO3 
E) NaNO3

Question 11

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Accepted Answer

The answer of 200.0 ml of a solution containing 0.5000...

Question 12

A buffer solution with a pH of 4.40 is prepared with 0.78 M Na C2H3O2 and ________ M HC2H3O2. The Ka of HC2H3O2 is 1.8 × 10-5.

Accepted Answer

A) 1.7 
B) 3.5 
C) 4.1 × 104 
D) 0.35 
E) 0.86

Question 13

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

Accepted Answer

The answer of Calculate the pH of a buffer that...

Question 14

In which one of the following solutions is silver chloride the most soluble?

Accepted Answer

A) 0.181 M HCl 
B) 0.0176 M NH3 
C) 0.744 M LiNO3 
D) pure water 
E) 0.181 M NaCl

Question 15

Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of sodium acetate in water sufficient to yield 1.00 L of solution. The Ka of acetic acid is 1.76 × 10-5.

Accepted Answer

A) 2.516 
B) 3.892 
C) 4.502 
D) 10.158 
E) 5.056

Question 16

Calculate the pH of a solution that is 0.278 M in sodium formate (NaHCO2)and 0.222 M in formic acid (HCO2H). The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A) 3.843 
B) 3.647 
C) 13.90 
D) 10.16 
E) 4.954

Question 17

Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.300 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10-5.

Accepted Answer

A) 5.204 
B) 4.300 
C) 9.700 
D) 8.781 
E) 8.796

Question 18

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 19

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

Accepted Answer

A) 0.0100 M KBr 
B) 0.040 M CuNO3 
C) 0.030 M NaBr 
D) 0.020 M LiBr 
E) CuBr will have the same solubility in all solutions.

Question 20

What is the pH of a buffer solution that is 0.266 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

Accepted Answer

A) 14.38 
B) 10.53 
C) 5.38 
D) 3.47 
E) 4.23

Exam 17: Additional Aspects of Aqueous Equilibria

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M hypochlorous acid to the equivalence point? The K_a of hypochlorous acid is 3.0 × 10^-8.

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

The K_bof ammonia is 1.76 × 10^-⁵. The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate is ________.

The primary buffer system that controls the pH of the blood is the ________ buffer system.

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The K_a of benzoic acid is 4.50 × 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 13.3 mL of base is added? The K_a of hypochlorous acid is 3.0 × 10^-8.

An assembly of a metal ion and the Lewis bases bonded to it is called a(n)________.

The addition of hydrochloric acid and ________ to water produces a buffer solution.

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

A buffer solution with a pH of 4.40 is prepared with 0.78 M Na C₂H₃O₂ and ________ M HC₂H₃O₂.The K_a of HC₂H₃O₂ is 1.8 × 10^-5.

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

In which one of the following solutions is silver chloride the most soluble?

Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of sodium acetate in water sufficient to yield 1.00 L of solution. The K_a of acetic acid is 1.76 × 10^-5.

Calculate the pH of a solution that is 0.278 M in sodium formate (NaHCO₂) and 0.222 M in formic acid (HCO₂H) . The K_a of formic acid is 1.77 × 10^-4.

Calculate the pH of a solution prepared by dissolving 0.850 mol of NH₃ and 0.300 mol of NH₄Cl in water sufficient to yield 1.00 L of solution. The K_b of ammonia is 1.77 × 10^-5.

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 of the following aqueous solutions would you expect CuBr to have the highest solubility?

What is the pH of a buffer solution that is 0.266 M in lactic acid and 0.111 M in sodium lactate? The K_a of lactic acid is 1.4 × 10^-4.

Exam 17: Additional Aspects of Aqueous Equilibria

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M hypochlorous acid to the equivalence point? The Ka of hypochlorous acid is 3.0 × 10-8.

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

The Kb of ammonia is 1.76 × 10-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate is ________.

The primary buffer system that controls the pH of the blood is the ________ buffer system.

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of benzoic acid is 4.50 × 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 13.3 mL of base is added? The Ka of hypochlorous acid is 3.0 × 10-8.

An assembly of a metal ion and the Lewis bases bonded to it is called a(n)________.

The addition of hydrochloric acid and ________ to water produces a buffer solution.

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

A buffer solution with a pH of 4.40 is prepared with 0.78 M Na C2H3O2 and ________ M HC2H3O2. The Ka of HC2H3O2 is 1.8 × 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.

In which one of the following solutions is silver chloride the most soluble?

Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of sodium acetate in water sufficient to yield 1.00 L of solution. The Ka of acetic acid is 1.76 × 10-5.

Calculate the pH of a solution that is 0.278 M in sodium formate (NaHCO2) and 0.222 M in formic acid (HCO2H) . The Ka of formic acid is 1.77 × 10-4.

Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.300 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10-5.

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 of the following aqueous solutions would you expect CuBr to have the highest solubility?

What is the pH of a buffer solution that is 0.266 M in lactic acid and 0.111 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M hypochlorous acid to the equivalence point? The K_a of hypochlorous acid is 3.0 × 10^-8.

The K_bof ammonia is 1.76 × 10^-⁵. The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate is ________.

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The K_a of benzoic acid is 4.50 × 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 13.3 mL of base is added? The K_a of hypochlorous acid is 3.0 × 10^-8.

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

A buffer solution with a pH of 4.40 is prepared with 0.78 M Na C₂H₃O₂ and ________ M HC₂H₃O₂.The K_a of HC₂H₃O₂ is 1.8 × 10^-5.

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

Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of sodium acetate in water sufficient to yield 1.00 L of solution. The K_a of acetic acid is 1.76 × 10^-5.

Calculate the pH of a solution that is 0.278 M in sodium formate (NaHCO₂) and 0.222 M in formic acid (HCO₂H) . The K_a of formic acid is 1.77 × 10^-4.

Calculate the pH of a solution prepared by dissolving 0.850 mol of NH₃ and 0.300 mol of NH₄Cl in water sufficient to yield 1.00 L of solution. The K_b of ammonia is 1.77 × 10^-5.

What is the pH of a buffer solution that is 0.266 M in lactic acid and 0.111 M in sodium lactate? The K_a of lactic acid is 1.4 × 10^-4.