A solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka = 6.3 × 10-5 for HC7H5O2. The solution volume is 5.00 L. What is the pH of the solution after 10.00 ml of 5.00 M NaOH is added?

A) 4.80 B) 4.86 C) 4.65 D) 4.70 E) 4.75 A) 4.80 B) 4.86 C) 4.65 D) 4.70 E) 4.75

A handbook states that to prepare a particular buffer solution mix 39.0 mL of 0.20 M NaH2PO4 with 61.0 mL of 0.20 M Na2HPO4. What will be the pH of this buffer?

A) 7.2 B) 7.4 C) 7.0 D) 6.8 E) 6.6 A) 7.2 B) 7.4 C) 7.0 D) 6.8 E) 6.6

In the neutralization of 50.0 mL of 0.1 M BOH (a weak base with Kb = 1.6 × 10-7) with 0.10 M H2SO4, the most correct description of the solution at the mid-point of the titration, i.e., half neutralized, is:

A) a solution in which [B+] essentially equals [BOH] B) a solution in which [B+] essentially equals 4 × 10-4 M C) a solution whose volume is 75 mL and contains some undissociated BOH molecules and some B+, OH-, and HSO4- ions D) a solution containing SO42- and B2+ ions E) a solution in contact with BSO4 solid A) a solution in which [B+] essentially equals [BOH] B) a solution in which [B+] essentially equals 4 × 10-4 M C) a solution whose volume is 75 mL and contains some undissociated BOH molecules and some B+, OH-, and HSO4- ions D) a solution containing SO42- and B2+ ions E) a solution in contact with BSO4 solid

If 30.0 mmol HCl(g) is added to 1.00 L of a buffer that is 0.340 M NH3(aq) and 0.290 M NH4Cl(aq), what are the final concentrations of NH3(aq) and NH4Cl(aq), respectively? Assume no volume change.

A) 0.310 M and 0.320 M B) 0.310 M and 0.290 M C) 0.370 M and 0.290 M D) 0.370 M and 0.320 M A) 0.310 M and 0.320 M B) 0.310 M and 0.290 M C) 0.370 M and 0.290 M D) 0.370 M and 0.320 M

Exam 17: Additional Aspects of Acid-Base Equilibria

A solution has [HC₇H₅O₂] = 0.100 M and [Ca(C₇H₅O₂)₂] = 0.200 M. Ka = 6.3 × 10^-5 for HC₇H₅O₂. The solution volume is 5.00 L. What is the pH of the solution after 10.00 ml of 5.00 M NaOH is added?

(Multiple Choice)

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Question 81

25 ml of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH before any NaOH is added? Ka for acetic acid = 1.8 × 10^-5.

(Multiple Choice)

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Question 82

A weak acid has Ka = 1.00 × 10^-3. If [HA] = 1.00 M what must be [A-] for the pH to be 2.7?

(Multiple Choice)

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Question 83

What factor governs the selection of an indicator for a neutralization titration?

(Multiple Choice)

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Question 84

A pH 9.56 buffer was prepared by mixing 2.00 moles of ammonia (Kb for ammonia is 1.8 × 10^-5) and 1.00 mol of ammonium chloride in water to form a solution with a volume of 1.00 L. To a 200.0 mL aliquot of this solution was added 10.0 mL of 10.0 M sodium hydroxide. What was the resulting pH?

(Multiple Choice)

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Question 85

A handbook states that to prepare a particular buffer solution mix 39.0 mL of 0.20 M NaH₂PO₄with 61.0 mL of 0.20 M Na₂HPO₄. What will be the pH of this buffer?

(Multiple Choice)

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Question 86

Twenty-five milliliters of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH after 15 ml of NaOH has been added?

(Multiple Choice)

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Question 87

In the neutralization of 50.0 mL of 0.1 M BOH (a weak base with Kb = 1.6 × 10^-7) with 0.10 M H₂SO₄, the most correct description of the solution at the mid-point of the titration, i.e., half neutralized, is:

(Multiple Choice)

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Question 88

How will addition of sodium chloride affect the pH of a HCl solution?

(Multiple Choice)

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Question 89

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0. State what color the indicator will assume in the following solution: 0.20 M KOH

(Multiple Choice)

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Question 90

Determine the [C₂H₃O₂^-] of the following solution. Initial concentrations are given. [HC₂H₃O₂] = 0.250 M, [HI] = 0.120 M [Ka = 1.8 × 10^-5]

(Multiple Choice)

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Question 91

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M ammonia (Kb = 1.8 × 10^-5). To this solution was then added 10.0 mL of 0.30 M sodium hydroxide, which caused a pH change of ________.

(Multiple Choice)

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Question 92

The Henderson-Hasselbach equation, used to calculate the pH of simple conjugate-pair buffer systems, would be expressed for an ammonia/ammonium chloride buffer, for which Kb(NH₃) is 1.8 × 10^-5, as:

(Multiple Choice)

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Question 93

The color change range of most acid-base indicators is 1 pH unit.

(True/False)

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Question 94

If 30.0 mmol HCl(g) is added to 1.00 L of a buffer that is 0.340 M NH₃(aq) and 0.290 M NH₄Cl(aq), what are the final concentrations of NH₃(aq) and NH₄Cl(aq), respectively? Assume no volume change.

(Multiple Choice)

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Question 95

What is the pH of a solution prepared by mixing equal volumes of 0.10 M hydrochloric and 0.1 M hydrofluoric acid? [Ka for HF is 6.6 × 10^-4]

(Multiple Choice)

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Question 96

Which of the following statements correctly describe a typical titration curve for the titration of a strong acid by a strong base? I. The beginning pH is low. II. The pH change is slow until near the equivalence point. III. At the equivalence point, pH changes by a large value. IV. Beyond the equivalence point, pH rises rapidly. V. The equivalence point would be at a pH less than 3.5.

(Multiple Choice)

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Question 97

The common ion in a mixture of a weak base and a strong base is the hydronium ion.

(True/False)

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Question 98

Determine the pH of the following solution. Initial concentrations are given. [NH₃] = 1.20 M, [KOH] = 0.320 M, Kb (NH₃) = 1.8 × 10^-5

(Multiple Choice)

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Question 99

Showing 81 - 99 of 99

Exam 17: Additional Aspects of Acid-Base Equilibria

A solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka = 6.3 × 10-5 for HC7H5O2. The solution volume is 5.00 L. What is the pH of the solution after 10.00 ml of 5.00 M NaOH is added?

25 ml of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH before any NaOH is added? Ka for acetic acid = 1.8 × 10-5.

A weak acid has Ka = 1.00 × 10-3. If [HA] = 1.00 M what must be [A-] for the pH to be 2.7?

What factor governs the selection of an indicator for a neutralization titration?

A pH 9.56 buffer was prepared by mixing 2.00 moles of ammonia (Kb for ammonia is 1.8 × 10-5) and 1.00 mol of ammonium chloride in water to form a solution with a volume of 1.00 L. To a 200.0 mL aliquot of this solution was added 10.0 mL of 10.0 M sodium hydroxide. What was the resulting pH?

A handbook states that to prepare a particular buffer solution mix 39.0 mL of 0.20 M NaH2PO4 with 61.0 mL of 0.20 M Na2HPO4. What will be the pH of this buffer?

Twenty-five milliliters of 0.10 M HCl is titrated with 0.10 M NaOH. What is the pH after 15 ml of NaOH has been added?

In the neutralization of 50.0 mL of 0.1 M BOH (a weak base with Kb = 1.6 × 10-7) with 0.10 M H2SO4, the most correct description of the solution at the mid-point of the titration, i.e., half neutralized, is:

How will addition of sodium chloride affect the pH of a HCl solution?

Phenol red indicator changes from yellow to red in the pH range from 6.6 to 8.0. State what color the indicator will assume in the following solution: 0.20 M KOH

Determine the [C2H3O2-] of the following solution. Initial concentrations are given. [HC2H3O2] = 0.250 M, [HI] = 0.120 M [Ka = 1.8 × 10-5]

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M ammonia (Kb = 1.8 × 10-5). To this solution was then added 10.0 mL of 0.30 M sodium hydroxide, which caused a pH change of ________.

The Henderson-Hasselbach equation, used to calculate the pH of simple conjugate-pair buffer systems, would be expressed for an ammonia/ammonium chloride buffer, for which Kb(NH3) is 1.8 × 10-5, as:

The color change range of most acid-base indicators is 1 pH unit.

If 30.0 mmol HCl(g) is added to 1.00 L of a buffer that is 0.340 M NH3(aq) and 0.290 M NH4Cl(aq), what are the final concentrations of NH3(aq) and NH4Cl(aq), respectively? Assume no volume change.

What is the pH of a solution prepared by mixing equal volumes of 0.10 M hydrochloric and 0.1 M hydrofluoric acid? [Ka for HF is 6.6 × 10-4]

The common ion in a mixture of a weak base and a strong base is the hydronium ion.

Determine the pH of the following solution. Initial concentrations are given. [NH3] = 1.20 M, [KOH] = 0.320 M, Kb (NH3) = 1.8 × 10-5

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A solution has [HC₇H₅O₂] = 0.100 M and [Ca(C₇H₅O₂)₂] = 0.200 M. Ka = 6.3 × 10^-5 for HC₇H₅O₂. The solution volume is 5.00 L. What is the pH of the solution after 10.00 ml of 5.00 M NaOH is added?

25 ml of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH before any NaOH is added? Ka for acetic acid = 1.8 × 10^-5.

A weak acid has Ka = 1.00 × 10^-3. If [HA] = 1.00 M what must be [A-] for the pH to be 2.7?

A pH 9.56 buffer was prepared by mixing 2.00 moles of ammonia (Kb for ammonia is 1.8 × 10^-5) and 1.00 mol of ammonium chloride in water to form a solution with a volume of 1.00 L. To a 200.0 mL aliquot of this solution was added 10.0 mL of 10.0 M sodium hydroxide. What was the resulting pH?

A handbook states that to prepare a particular buffer solution mix 39.0 mL of 0.20 M NaH₂PO₄with 61.0 mL of 0.20 M Na₂HPO₄. What will be the pH of this buffer?

In the neutralization of 50.0 mL of 0.1 M BOH (a weak base with Kb = 1.6 × 10^-7) with 0.10 M H₂SO₄, the most correct description of the solution at the mid-point of the titration, i.e., half neutralized, is:

Determine the [C₂H₃O₂^-] of the following solution. Initial concentrations are given. [HC₂H₃O₂] = 0.250 M, [HI] = 0.120 M [Ka = 1.8 × 10^-5]

A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M ammonia (Kb = 1.8 × 10^-5). To this solution was then added 10.0 mL of 0.30 M sodium hydroxide, which caused a pH change of ________.

The Henderson-Hasselbach equation, used to calculate the pH of simple conjugate-pair buffer systems, would be expressed for an ammonia/ammonium chloride buffer, for which Kb(NH₃) is 1.8 × 10^-5, as:

If 30.0 mmol HCl(g) is added to 1.00 L of a buffer that is 0.340 M NH₃(aq) and 0.290 M NH₄Cl(aq), what are the final concentrations of NH₃(aq) and NH₄Cl(aq), respectively? Assume no volume change.

What is the pH of a solution prepared by mixing equal volumes of 0.10 M hydrochloric and 0.1 M hydrofluoric acid? [Ka for HF is 6.6 × 10^-4]

Determine the pH of the following solution. Initial concentrations are given. [NH₃] = 1.20 M, [KOH] = 0.320 M, Kb (NH₃) = 1.8 × 10^-5