Question 1

What is the pH after the addition of 0.20 mole of HCl to 1.00 liter of 1.00 M CH3COONa and 1.00 M CH3COOH ( K a = 1.8×10 - 5) buffer solution?
(Assume no volume change.)

Accepted Answer

A)  0.70 
B)  2.31 
C)  4.57 
D)  9.28 
E)  13.3

Question 2

The pH at the equivalence point in the titration of 0.10 M NH3 with 0.10 M HCl is:

Accepted Answer

A)  strongly acidic. 
B)  slightly acidic. 
C)  neutral (pH 7.0). 
D)  slightly basic. 
E)  strongly basic.

Question 3

How many grams of sodium acetate, CH3COONa, is required to mix witH₂ .00 Liters of 0.450 M acetic acid, CH3COOH, in order to prepare a buffer solution with a pH that equals 5.00?
P K a(CH3COOH) = 4.74 and MM(CH3COONa) = 82.03 g/mol

Accepted Answer

A)  2.00×10 - 2 g CH3COONa 
B)  45.6 g CH3COONa 
C)  67.2 g CH3COONa 
D)  134 g CH3COONa 
E)  299 g CH3COONa

Question 4

A sample of ammonia (approximately 0.10 M, K b = 1.8×10 - 5) is titrated with 0.0993 M HCl. What indicator should be used?

Accepted Answer

A)  methyl red (p K In = 5.00) 
B)  bromthymol blue (p K In = 7.30) 
C)  phenolphthalein (p K In = 8.7) 
D)  thymol blue (p K In = 9.20) 
E)  alizarin yellow R (p K In = 10.2)

Question 5

In the titration of 25.0 mL of 0.100 M acetic acid ( K a = 1.8×10 - 5) with 0.100 M NaOH, the pH after adding 12.5 mL of titrant is:

Accepted Answer

A)  12.52 
B)  3.50 
C)  7.00 
D)  4.74 
E)  2.38

Question 6

What is the pH of a buffer solution that consists of 0.83 M HBrO and 0.53 M KBrO?
K a(HBrO) = 2.3×10 - 9

Accepted Answer

A)  pH = 8.19 
B)  pH = 8.45 
C)  pH = 8.83 
D)  pH = 8.93 
E)  pH = 12.05

Question 7

What is the concentration of ammonium ion, [NH4+], present at equilibrium if 0.100 moles of NaOH are added to 0.200 moles of NH3 to form one-liter of solution?

Accepted Answer

A)  [NH4+] = 9.0×10 - 6 M 
B)  [NH4+] = 3.6×10 - 5 M 
C)  [NH4+] = 1.9×10 - 3 M 
D)  [NH4+] = 6.0×10 - 3 M 
E)  [NH4+] = 0.10 M

Question 8

The sharpest inflection point is observed in the titration of

Accepted Answer

A)  0.1 M HCl with 0.10 M NaOH 
B)  0.01 M HCl with 0.10 M NaOH 
C)  0.1 M KOH with 0.10 M NaOH 
D)  0.1 M HF ( Ka = 3.5×10 - 4) with 0.10 M NaOH 
E)  0.10 M NH3 with 0.10 M NaOH

Question 9

In the titration of 0.100 M HCl with the titrant 0.100 M NaOH, what species are present after the equivalence point?

Accepted Answer

A)  HCl only 
B)  NaOH only 
C)  NaCl only 
D)  NaOH and NaCl 
E)  HCl and NaCl

Question 10

The titration of a weak acid, HA ( K a = 1.0×10 - 4), with NaOH requires 40.0 mL to reach the equivalence point. The pH after 20 mL is

Accepted Answer

A)  Strongly alkaline, approximately 12 
B)  Moderately alkaline, approximately 10 
C)  Slightly alkaline, approximately 8 
D)  Neutral, approximately 7 
E)  Moderately acidic, approximately 4

Question 11

What is the pH of solution formed by adding 25.0 mL of 0.100 M HCl to 25.0 mL of 0.100 M pyridine (C5H5N, K b = 1.8×10 - 9)?

Accepted Answer

A)  2.38 
B)  2.52 
C)  2.98 
D)  3.28 
E)  8.74

Question 12

Consider the ionization of acetic acid as follows:CH ₃COOH + H₂ O  H₃O + + CH₃COO 1 - What is the effect of adding the common ion, acetate, CH₃COO - (source:
CH₃COONa), to this equilibrium system?

Accepted Answer

A)  The equilibrium shifts to the left and the pH rises. 
B)  The equilibrium shifts to the right and the pH rises. 
C)  The equilibrium shifts to the left and the pH lowers. 
D)  The equilibrium shifts to the right and the pH lowers. 
E)  Nothing happens. The pH remains constant and the equilibrium does not shift in either direction.

Question 13

Exhibit 16-3 Consider the Titration curve below for the titration of a weak acid ,CH ₃COOH , with a strong base , NaOH, to answer the following question(s). CH ₃COOH + NaOH CH ₃COONa + H₂ O 
Refer to Exhibit 16-3. What approach listed below would be used to determine the pH at point A of the solution?

Accepted Answer

A)  This is a problem of solving for the pH of an aqueous weak acid solution. 
B)  This is a problem of solving for the pH of an aqueous weak base solution. 
C)  This is a problem of solving for the pH of an aqueous buffer solution. 
D)  This is a problem of solving for the pH of an aqueous strong base solution. 
E)  This is a problem of solving for the pH of an aqueous salt solution.

Question 14

A solution is made by dissolving 0.100 mole NH3 ( K b = 1.8×10 - 5) and 0.200 mole of NH4Cl in water and diluting to 1.00 L. What is the pH of the resulting solution?

Accepted Answer

A)  8.95 
B)  11.12 
C)  2.72 
D)  13.00 
E)  5.04

Question 15

Calculate the pH at the equivalence point for the titration of 20.0 mL of 1.00 M HF with 0.500 M NaOH. K a = 3.5×10 - 4 for HF.

Accepted Answer

A)  1.73 
B)  5.53 
C)  12.3 
D)  7.00 
E)  8.49

Question 16

Carbonic acid is a diprotic acid with K al = 4.3×10 - 7 and K a2 = 5.6×10 - 11. What is K b for the carbonate ion, CO32 - ?

Accepted Answer

A)  5.6×103 
B)  5.6×10 - 3 
C)  1.8×10 - 4 
D)  4.3×10 - 7 
E)  2.3×10 - 8

Question 17

A sample of hydrochloric acid (approximately 0.10 M) is titrated with 0.0993 M NaOH. What indicator changes color closest to the equivalence point?

Accepted Answer

A)  thymol blue (p K In = 1.65) 
B)  methyl orange (p K In = 3.46) 
C)  methyl red (p K In = 5.00) 
D)  bromthymol blue (p K In = 7.30) 
E)  phenolphthalein (p K In = 8.7)

Question 18

The titration of a weak base ( K b = 1.0×10 - 4) with HCl requires 40.0 mL to reach the equivalence point. In order to calculate the pH of the system after 20 mL of HCl is added, the best strategy is to recognize that the system is

Accepted Answer

A)  a strong base 
B)  a weak base 
C)  a buffer 
D)  neutral 
E)  a strong acid

Exam 16: Reactions Between Acids and Bases

What is the pH after the addition of 0.20 mole of HCl to 1.00 liter of 1.00 M CH₃COONa and 1.00 M CH₃COOH ( K _a = 1.8×10^{- 5}) buffer solution? (Assume no volume change.)

The pH at the equivalence point in the titration of 0.10 M NH₃ with 0.10 M HCl is:

How many grams of sodium acetate, CH₃COONa, is required to mix witH₂ .00 Liters of 0.450 M acetic acid, CH₃COOH, in order to prepare a buffer solution with a pH that equals 5.00? P K _a(CH₃COOH) = 4.74 and MM(CH₃COONa) = 82.03 g/mol

A sample of ammonia (approximately 0.10 M, K _b = 1.8×10^{- 5}) is titrated with 0.0993 M HCl. What indicator should be used?

In the titration of 25.0 mL of 0.100 M acetic acid ( K _a = 1.8×10^{- 5}) with 0.100 M NaOH, the pH after adding 12.5 mL of titrant is:

What is the pH of a buffer solution that consists of 0.83 M HBrO and 0.53 M KBrO? K _a(HBrO) = 2.3×10^{- 9}

What is the concentration of ammonium ion, [NH₄⁺], present at equilibrium if 0.100 moles of NaOH are added to 0.200 moles of NH₃ to form one-liter of solution?

The sharpest inflection point is observed in the titration of

In the titration of 0.100 M HCl with the titrant 0.100 M NaOH, what species are present after the equivalence point?

The titration of a weak acid, HA ( K _a = 1.0×10^{- 4}) , with NaOH requires 40.0 mL to reach the equivalence point. The pH after 20 mL is

What is the pH of solution formed by adding 25.0 mL of 0.100 M HCl to 25.0 mL of 0.100 M pyridine (C₅H₅N, K _b = 1.8×10^{- 9}) ?

Consider the ionization of acetic acid as follows:CH ₃COOH + H₂ O H₃O + + CH₃COO 1 - What is the effect of adding the common ion, acetate, CH₃COO - (source: CH₃COONa) , to this equilibrium system?

A solution is made by dissolving 0.100 mole NH₃ ( K _b = 1.8×10^{- 5}) and 0.200 mole of NH₄Cl in water and diluting to 1.00 L. What is the pH of the resulting solution?

Calculate the pH at the equivalence point for the titration of 20.0 mL of 1.00 M HF with 0.500 M NaOH. K _a = 3.5×10^{- 4} for HF.

Carbonic acid is a diprotic acid with K _al = 4.3×10^{- 7} and K _a2 = 5.6×10^{- 11}. What is K _b for the carbonate ion, CO₃^{2 -}?

A sample of hydrochloric acid (approximately 0.10 M) is titrated with 0.0993 M NaOH. What indicator changes color closest to the equivalence point?

The titration of a weak base ( K _b = 1.0×10^{- 4}) with HCl requires 40.0 mL to reach the equivalence point. In order to calculate the pH of the system after 20 mL of HCl is added, the best strategy is to recognize that the system is

Exam 16: Reactions Between Acids and Bases

What is the pH after the addition of 0.20 mole of HCl to 1.00 liter of 1.00 M CH3COONa and 1.00 M CH3COOH ( K a = 1.8×10 - 5) buffer solution? (Assume no volume change.)

The pH at the equivalence point in the titration of 0.10 M NH3 with 0.10 M HCl is:

How many grams of sodium acetate, CH3COONa, is required to mix witH₂ .00 Liters of 0.450 M acetic acid, CH3COOH, in order to prepare a buffer solution with a pH that equals 5.00? P K a(CH3COOH) = 4.74 and MM(CH3COONa) = 82.03 g/mol

A sample of ammonia (approximately 0.10 M, K b = 1.8×10 - 5) is titrated with 0.0993 M HCl. What indicator should be used?

In the titration of 25.0 mL of 0.100 M acetic acid ( K a = 1.8×10 - 5) with 0.100 M NaOH, the pH after adding 12.5 mL of titrant is:

What is the pH of a buffer solution that consists of 0.83 M HBrO and 0.53 M KBrO? K a(HBrO) = 2.3×10 - 9

What is the concentration of ammonium ion, [NH4+], present at equilibrium if 0.100 moles of NaOH are added to 0.200 moles of NH3 to form one-liter of solution?

The sharpest inflection point is observed in the titration of

In the titration of 0.100 M HCl with the titrant 0.100 M NaOH, what species are present after the equivalence point?

The titration of a weak acid, HA ( K a = 1.0×10 - 4) , with NaOH requires 40.0 mL to reach the equivalence point. The pH after 20 mL is

What is the pH of solution formed by adding 25.0 mL of 0.100 M HCl to 25.0 mL of 0.100 M pyridine (C5H5N, K b = 1.8×10 - 9) ?

Consider the ionization of acetic acid as follows:CH ₃COOH + H₂ O H₃O + + CH₃COO 1 - What is the effect of adding the common ion, acetate, CH₃COO - (source: CH₃COONa) , to this equilibrium system?

A solution is made by dissolving 0.100 mole NH3 ( K b = 1.8×10 - 5) and 0.200 mole of NH4Cl in water and diluting to 1.00 L. What is the pH of the resulting solution?

Calculate the pH at the equivalence point for the titration of 20.0 mL of 1.00 M HF with 0.500 M NaOH. K a = 3.5×10 - 4 for HF.

Carbonic acid is a diprotic acid with K al = 4.3×10 - 7 and K a2 = 5.6×10 - 11. What is K b for the carbonate ion, CO32 - ?

A sample of hydrochloric acid (approximately 0.10 M) is titrated with 0.0993 M NaOH. What indicator changes color closest to the equivalence point?

The titration of a weak base ( K b = 1.0×10 - 4) with HCl requires 40.0 mL to reach the equivalence point. In order to calculate the pH of the system after 20 mL of HCl is added, the best strategy is to recognize that the system is

What is the pH after the addition of 0.20 mole of HCl to 1.00 liter of 1.00 M CH₃COONa and 1.00 M CH₃COOH ( K _a = 1.8×10^{- 5}) buffer solution? (Assume no volume change.)

The pH at the equivalence point in the titration of 0.10 M NH₃ with 0.10 M HCl is:

How many grams of sodium acetate, CH₃COONa, is required to mix witH₂ .00 Liters of 0.450 M acetic acid, CH₃COOH, in order to prepare a buffer solution with a pH that equals 5.00? P K _a(CH₃COOH) = 4.74 and MM(CH₃COONa) = 82.03 g/mol

A sample of ammonia (approximately 0.10 M, K _b = 1.8×10^{- 5}) is titrated with 0.0993 M HCl. What indicator should be used?

In the titration of 25.0 mL of 0.100 M acetic acid ( K _a = 1.8×10^{- 5}) with 0.100 M NaOH, the pH after adding 12.5 mL of titrant is:

What is the pH of a buffer solution that consists of 0.83 M HBrO and 0.53 M KBrO? K _a(HBrO) = 2.3×10^{- 9}

What is the concentration of ammonium ion, [NH₄⁺], present at equilibrium if 0.100 moles of NaOH are added to 0.200 moles of NH₃ to form one-liter of solution?

The titration of a weak acid, HA ( K _a = 1.0×10^{- 4}) , with NaOH requires 40.0 mL to reach the equivalence point. The pH after 20 mL is

What is the pH of solution formed by adding 25.0 mL of 0.100 M HCl to 25.0 mL of 0.100 M pyridine (C₅H₅N, K _b = 1.8×10^{- 9}) ?

A solution is made by dissolving 0.100 mole NH₃ ( K _b = 1.8×10^{- 5}) and 0.200 mole of NH₄Cl in water and diluting to 1.00 L. What is the pH of the resulting solution?

Calculate the pH at the equivalence point for the titration of 20.0 mL of 1.00 M HF with 0.500 M NaOH. K _a = 3.5×10^{- 4} for HF.

Carbonic acid is a diprotic acid with K _al = 4.3×10^{- 7} and K _a2 = 5.6×10^{- 11}. What is K _b for the carbonate ion, CO₃^{2 -}?

The titration of a weak base ( K _b = 1.0×10^{- 4}) with HCl requires 40.0 mL to reach the equivalence point. In order to calculate the pH of the system after 20 mL of HCl is added, the best strategy is to recognize that the system is