What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 mol L-1 NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

A) 9.08 B) 9.26 C) 9.43 D) 11.32 A) 9.08 B) 9.26 C) 9.43 D) 11.32 C

What is the pH of the resulting solution if 45 mL of 0.432 mol L-1 aqueous methylamine,CH3NH2,is added to 15 mL of 0.234 mol L-1 HCl(aq)? Assume that the volumes of the solutions are additive.Ka = 2.70 × 10-11 for CH3NH3+.

A) 2.77 B) 4.09 C) 9.91 D) 11.23 A) 2.77 B) 4.09 C) 9.91 D) 11.23

Calculate the pH of a 1.00 L solution of 0.100 M NH3(aq)after the addition of 0.010 mol NH4Cl(s).For NH3,pKb = 4.74.

A) 10.26 B) 9.26 C) 8.26 D) 11.56 A) 10.26 B) 9.26 C) 8.26 D) 11.56

If 25 mL of 0.20 M NaOH(aq)is added to 50 mL of 0.10 M aqueous HC2H3O2 (Ka = 1.8 × 10-5),what is the pH?

A) 5.33 B) 10.21 C) 8.78 D) 13.56 E) 1.34 A) 5.33 B) 10.21 C) 8.78 D) 13.56 E) 1.34

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L-1 NH3 with 5.00 mL of 0.10 mol L-1 NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

A) 8.25 B) 9.28 C) 10.26 D) 11.13 A) 8.25 B) 9.28 C) 10.26 D) 11.13

Calculate the pH of an aqueous solution that is 1.0 M Na2CO3.Ka2 for H2CO3 is 4.7 × 10-11.

A) 8.8 B) 10.3 C) 3.7 D) 12.2 E) 1.8 A) 8.8 B) 10.3 C) 3.7 D) 12.2 E) 1.8

Exam 17: Additional Aspects of Acidbase Equilibria

What mass of sodium acetate should be dissolved in 250.0 mL of 0.30 M aqueous acetic acid to form a buffer of pH 5.0? (K_a for acetic acid is 1.8 × 10^-5)

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Question 1

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What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

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Question 2

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25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq).What is the pH at the equivalence point? K_a for acetic acid = 1.8 × 10^-5.

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Question 3

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Why do we avoid titrating ammonia with acetic acid?

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Question 4

In the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq)with 0.100 M NaOH(aq),what is/are the major species in the solution after the addition of 5.0 mL of NaOH(aq)?

(Multiple Choice)

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Question 5

What is the pH of the resulting solution if 45 mL of 0.432 mol L^-1 aqueous methylamine,CH₃NH₂,is added to 15 mL of 0.234 mol L^-1 HCl(aq)? Assume that the volumes of the solutions are additive.K_a = 2.70 × 10^-11for CH₃NH₃⁺.

(Multiple Choice)

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Question 6

Calculate the pH of a 1.00 L solution of 0.100 M NH₃(aq)after the addition of 0.010 mol NH₄Cl(s).For NH₃,pK_b = 4.74.

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Question 7

If 25 mL of 0.20 M NaOH(aq)is added to 50 mL of 0.10 M aqueous HC₂H₃O₂(K_a = 1.8 × 10^-5),what is the pH?

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Question 8

An acid has a K_a = 1 × 10^-6.At what pH would this acid and its corresponding salt make a good buffer?

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Question 9

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 NH₃ with 5.00 mL of 0.10 mol L^-1 NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

(Multiple Choice)

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Question 10

What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH3COOH.

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Question 11

Which among the following pairs is inefficient as buffer pair?

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Question 12

Twenty-five milliliters of 0.10 M HCl(aq)is titrated with 0.10 M NaOH(aq).What is the pH when 30 mL of NaOH(aq)have been added?

(Multiple Choice)

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Question 13

Calculate the pH of an aqueous solution that is 0.210 mol L^-1 in nitrous acid ( ) and 0.290 mol L^-1 in potassium nitrite ( ).The acid dissociation constant of nitrous acid is 4.50 × .

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Question 14

Determine the [F^-] of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[NaF] = 1.045 M,K_a for HF is 6.6 × 10^-4

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Question 15

The pH of a buffer solution changes only slightly with addition of a small amount of acid or base.

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Question 16

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

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Question 17

What is the pH of a 0.30 M aqueous trisodium phosphate solution? K_a for monohydrogen phosphate ion is 4.2 × 10^-13

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Question 18

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.

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Question 19

Calculate the pH of an aqueous solution that is 1.0 M Na₂CO₃.K_a2 for H₂CO₃ is 4.7 × 10^-11.

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Question 20

Showing 1 - 20 of 130

Exam 17: Additional Aspects of Acidbase Equilibria

What mass of sodium acetate should be dissolved in 250.0 mL of 0.30 M aqueous acetic acid to form a buffer of pH 5.0? (Ka for acetic acid is 1.8 × 10-5)

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 mol L-1 NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq).What is the pH at the equivalence point? Ka for acetic acid = 1.8 × 10-5.

Why do we avoid titrating ammonia with acetic acid?

In the titration of 50.0 mL of 0.0200 M C6H5COOH(aq)with 0.100 M NaOH(aq),what is/are the major species in the solution after the addition of 5.0 mL of NaOH(aq)?

What is the pH of the resulting solution if 45 mL of 0.432 mol L-1 aqueous methylamine,CH3NH2,is added to 15 mL of 0.234 mol L-1 HCl(aq)? Assume that the volumes of the solutions are additive.Ka = 2.70 × 10-11 for CH3NH3+.

Calculate the pH of a 1.00 L solution of 0.100 M NH3(aq)after the addition of 0.010 mol NH4Cl(s).For NH3,pKb = 4.74.

If 25 mL of 0.20 M NaOH(aq)is added to 50 mL of 0.10 M aqueous HC2H3O2 (Ka = 1.8 × 10-5),what is the pH?

An acid has a Ka = 1 × 10-6.At what pH would this acid and its corresponding salt make a good buffer?

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L-1 NH3 with 5.00 mL of 0.10 mol L-1 NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

What is the [CH3COO-]/[CH3COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34? Ka = 1.8 × 10-5 for CH3COOH.

Which among the following pairs is inefficient as buffer pair?

Twenty-five milliliters of 0.10 M HCl(aq)is titrated with 0.10 M NaOH(aq).What is the pH when 30 mL of NaOH(aq)have been added?

Calculate the pH of an aqueous solution that is 0.210 mol L-1 in nitrous acid ( ) and 0.290 mol L-1 in potassium nitrite ( ).The acid dissociation constant of nitrous acid is 4.50 × .

Determine the [F-] of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[NaF] = 1.045 M,Ka for HF is 6.6 × 10-4

The pH of a buffer solution changes only slightly with addition of a small amount of acid or base.

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

What is the pH of a 0.30 M aqueous trisodium phosphate solution? Ka for monohydrogen phosphate ion is 4.2 × 10-13

Calculate the pH of an aqueous solution that is 1.0 M Na2CO3.Ka2 for H2CO3 is 4.7 × 10-11.

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What mass of sodium acetate should be dissolved in 250.0 mL of 0.30 M aqueous acetic acid to form a buffer of pH 5.0? (K_a for acetic acid is 1.8 × 10^-5)

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

25 mL of 0.10 M aqueous acetic acid is titrated with 0.10 M NaOH(aq).What is the pH at the equivalence point? K_a for acetic acid = 1.8 × 10^-5.

In the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq)with 0.100 M NaOH(aq),what is/are the major species in the solution after the addition of 5.0 mL of NaOH(aq)?

What is the pH of the resulting solution if 45 mL of 0.432 mol L^-1 aqueous methylamine,CH₃NH₂,is added to 15 mL of 0.234 mol L^-1 HCl(aq)? Assume that the volumes of the solutions are additive.K_a = 2.70 × 10^-11for CH₃NH₃⁺.

Calculate the pH of a 1.00 L solution of 0.100 M NH₃(aq)after the addition of 0.010 mol NH₄Cl(s).For NH₃,pK_b = 4.74.

If 25 mL of 0.20 M NaOH(aq)is added to 50 mL of 0.10 M aqueous HC₂H₃O₂(K_a = 1.8 × 10^-5),what is the pH?

An acid has a K_a = 1 × 10^-6.At what pH would this acid and its corresponding salt make a good buffer?

What is the pH of an aqueous solution prepared by mixing 50.00 mL of 0.10 mol L^-1 NH₃ with 5.00 mL of 0.10 mol L^-1 NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH3COOH.

Calculate the pH of an aqueous solution that is 0.210 mol L^-1 in nitrous acid ( ) and 0.290 mol L^-1 in potassium nitrite ( ).The acid dissociation constant of nitrous acid is 4.50 × .

Determine the [F^-] of the following aqueous solution.Initial concentrations are given. [HF] = 1.296 M,[NaF] = 1.045 M,K_a for HF is 6.6 × 10^-4

What is the pH of a 0.30 M aqueous trisodium phosphate solution? K_a for monohydrogen phosphate ion is 4.2 × 10^-13

Calculate the pH of an aqueous solution that is 1.0 M Na₂CO₃.K_a2 for H₂CO₃ is 4.7 × 10^-11.