What is the pH of a solution that consists of 0.25 M HC2H3O2 and 0.35 M NaC2H3O2? K a(HC2H3O2) = 1.8×10 - 5

A) 0.60 B) 4.60 C) 4.89 D) 5.50 E) 6.07 A) 0.60 B) 4.60 C) 4.89 D) 5.50 E) 6.07 C

What is the pH of a solution that is 0.100 M methylamine (CH3NH2) and 0.200 M methyl ammonium chloride (CH3NH3Cl)? The K b of methylamine is 3.70×10 - 4.

A) 1.00 B) 3.73 C) 10.73 D) 3.43 E) 10.27 A) 1.00 B) 3.73 C) 10.73 D) 3.43 E) 10.27

Calculate the number of moles of sodium acetate (CH3COONa) that must be added to 1.00 L of 0.100 M CH3COOH ( K a = 1.8×10 - 5) to give a buffer with pH5.00.

A) 1.0×10 - 5 B) 0.18 C) 0.057 D) 0.10 E) 0.20 A) 1.0×10 - 5 B) 0.18 C) 0.057 D) 0.10 E) 0.20

What is the pH of a buffer solution that consists of 0.25 M HClO2 and 0.75 M KClO2? K a(HClO2) = 1.1×10 - 2

A) pH = 1.48 B) pH = 1.96 C) pH = 2.44 D) pH = 3.41 E) pH = 5.61 A) pH = 1.48 B) pH = 1.96 C) pH = 2.44 D) pH = 3.41 E) pH = 5.61

What is the pH of a solution prepared by mixing 0.250 mol of hydrazoic acid, HN3, and 0.500 mol of sodium azide, NaN3, to make 1.00 liter of solution? ( K a = 1.9×10 - 5)

A) 4.42 B) 5.02 C) 9.58 D) 4.72 E) 8.98 A) 4.42 B) 5.02 C) 9.58 D) 4.72 E) 8.98

Exam 16: Reactions Between Acids and Bases

Consider titrating a triprotic acid with standard NaOH as shown in the titration curve below. What is the relationship between the first equivalence point and the third equivalence point in this titration curve?

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(Multiple Choice)

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Question 1

Correct Answer:

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Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution? I. Fe(OH)₃ II. AgCN III. PbI₂

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Question 2

Correct Answer:

Verified

What is the pH of a solution that consists of 0.25 M HC₂H₃O₂ and 0.35 M NaC₂H₃O₂? K _a(HC₂H₃O₂) = 1.8×10^{- 5}

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Question 3

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Verified

What is the pH of a solution that is 0.100 M methylamine (CH₃NH₂) and 0.200 M methyl ammonium chloride (CH₃NH₃Cl)? The K _b of methylamine is 3.70×10^{- 4}.

(Multiple Choice)

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Question 4

Calculate the volume of 0.100 M HCl required to neutralize 1.00 g of Ba(OH)₂ (molar mass = 171.3 g/mol).

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Question 5

Consider the buffer pair, HF/F^-. What can be stated about the relative proportions of this buffer pair if the pH of an aqueous solution of this pair is adjusted tO₄.00 and the p K _a for HF equals 3.17?

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Question 6

A 20.0 mL sample of lactic acid (monoprotic with K _a = 1.37×10^{- 4}) requires 30.0 mL of 0.200 M NaOH for titration to the equivalence point. What is the concentration of the lactic acid solution?

(Multiple Choice)

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Question 7

A buffer solution maintains a constant pH level to a certain extent when a strong acid such as HCl is added. Which of the following buffer solutions has the greatest buffering capacity to consume added HCl?

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Question 8

In the titration of 50.0 mL of a 0.100 M HCl solution with 0.100 M NaOH, what is the pH of the solution after the addition of 20.0 mL of the NaOH solution?

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Question 9

Which of the following titration curves listed below best represents a curve for the complete titration of oxalic acid, H₂C₂O₄ (a diprotic acid), with a strong base such as NaOH?

(Multiple Choice)

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Question 10

Exhibit 16-2 Consider titrating CH₃COOH with standard NaOH (delivered from the burette) to answer the following question(s). -Refer to Exhibit 16-2. What compound(s) is(are) present in the region after the titration has begun but before the equivalence point? I. CH₃COOH II. NaOH III. CH₃COO^-Na⁺

(Multiple Choice)

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Question 11

A 350 mL volume of 0.150 M Ba(OH)₂ was completely neutralized by 35.0 mL of HCl. What is the molarity of the HCl solution?

(Multiple Choice)

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Question 12

A buffer is made by dissolving 0.10 mol of NaF in 1.00 L of 0.20 M HF. What is the pH of this buffer? K _a(HF) = 6.3×10^{- 4}

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Question 13

In the titration of 0.100 M HCl with the titrant 0.100 M NaOH, what species are present at any point after NaOH has been added but before the equivalence point?

(Multiple Choice)

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Question 14

Which of the following titration curves listed below best represents a curve for the complete titration of the weakly basic dianion, sulfide, S^{2 -}, with a strong acid such as HCl as shown below in the net ionic equation? S^{2 -} (aq) + 2 HCl (aq)→H₂S (g) + 2 Cl^-

(Multiple Choice)

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Question 15

Calculate the number of moles of sodium acetate (CH₃COONa) that must be added to 1.00 L of 0.100 M CH₃COOH ( K _a = 1.8×10^{- 5}) to give a buffer with pH₅.00.

(Multiple Choice)

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Question 16

Calculate the pH of a solution after 10.0 mL of 0.100 M NaOH is added tO₄0.0 mL of 0.250 M HBr.

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Question 17

What is the pH of a buffer solution that consists of 0.25 M HClO₂ and 0.75 M KClO₂? K _a(HClO₂) = 1.1×10^{- 2}

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Question 18

Which pair(s) of substances would make a suitable buffer pair ? I. HCl and NaCl II. HF and NaF III. NH₄Cl and NH₃

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Question 19

What is the pH of a solution prepared by mixing 0.250 mol of hydrazoic acid, HN₃, and 0.500 mol of sodium azide, NaN₃, to make 1.00 liter of solution? ( K _a = 1.9×10^{- 5})

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Question 20

Showing 1 - 20 of 98

Exam 16: Reactions Between Acids and Bases

Consider titrating a triprotic acid with standard NaOH as shown in the titration curve below. What is the relationship between the first equivalence point and the third equivalence point in this titration curve?

Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution? I. Fe(OH)3 II. AgCN III. PbI2

What is the pH of a solution that consists of 0.25 M HC2H3O2 and 0.35 M NaC2H3O2? K a(HC2H3O2) = 1.8×10 - 5

What is the pH of a solution that is 0.100 M methylamine (CH3NH2) and 0.200 M methyl ammonium chloride (CH3NH3Cl)? The K b of methylamine is 3.70×10 - 4.

Calculate the volume of 0.100 M HCl required to neutralize 1.00 g of Ba(OH)2 (molar mass = 171.3 g/mol).

Consider the buffer pair, HF/F - . What can be stated about the relative proportions of this buffer pair if the pH of an aqueous solution of this pair is adjusted tO4.00 and the p K a for HF equals 3.17?

A 20.0 mL sample of lactic acid (monoprotic with K a = 1.37×10 - 4) requires 30.0 mL of 0.200 M NaOH for titration to the equivalence point. What is the concentration of the lactic acid solution?

A buffer solution maintains a constant pH level to a certain extent when a strong acid such as HCl is added. Which of the following buffer solutions has the greatest buffering capacity to consume added HCl?

In the titration of 50.0 mL of a 0.100 M HCl solution with 0.100 M NaOH, what is the pH of the solution after the addition of 20.0 mL of the NaOH solution?

Which of the following titration curves listed below best represents a curve for the complete titration of oxalic acid, H2C2O4 (a diprotic acid), with a strong base such as NaOH?

Exhibit 16-2 Consider titrating CH3COOH with standard NaOH (delivered from the burette) to answer the following question(s). -Refer to Exhibit 16-2. What compound(s) is(are) present in the region after the titration has begun but before the equivalence point? I. CH3COOH II. NaOH III. CH3COO - Na+

A 350 mL volume of 0.150 M Ba(OH)2 was completely neutralized by 35.0 mL of HCl. What is the molarity of the HCl solution?

A buffer is made by dissolving 0.10 mol of NaF in 1.00 L of 0.20 M HF. What is the pH of this buffer? K a(HF) = 6.3×10 - 4

In the titration of 0.100 M HCl with the titrant 0.100 M NaOH, what species are present at any point after NaOH has been added but before the equivalence point?

Which of the following titration curves listed below best represents a curve for the complete titration of the weakly basic dianion, sulfide, S2 - , with a strong acid such as HCl as shown below in the net ionic equation? S2 - (aq) + 2 HCl (aq)→H2S (g) + 2 Cl -

Calculate the number of moles of sodium acetate (CH3COONa) that must be added to 1.00 L of 0.100 M CH3COOH ( K a = 1.8×10 - 5) to give a buffer with pH5.00.

Calculate the pH of a solution after 10.0 mL of 0.100 M NaOH is added tO40.0 mL of 0.250 M HBr.

What is the pH of a buffer solution that consists of 0.25 M HClO2 and 0.75 M KClO2? K a(HClO2) = 1.1×10 - 2

Which pair(s) of substances would make a suitable buffer pair ? I. HCl and NaCl II. HF and NaF III. NH4Cl and NH3

What is the pH of a solution prepared by mixing 0.250 mol of hydrazoic acid, HN3, and 0.500 mol of sodium azide, NaN3, to make 1.00 liter of solution? ( K a = 1.9×10 - 5)

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Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution? I. Fe(OH)₃ II. AgCN III. PbI₂

What is the pH of a solution that consists of 0.25 M HC₂H₃O₂ and 0.35 M NaC₂H₃O₂? K _a(HC₂H₃O₂) = 1.8×10^{- 5}

What is the pH of a solution that is 0.100 M methylamine (CH₃NH₂) and 0.200 M methyl ammonium chloride (CH₃NH₃Cl)? The K _b of methylamine is 3.70×10^{- 4}.

Calculate the volume of 0.100 M HCl required to neutralize 1.00 g of Ba(OH)₂ (molar mass = 171.3 g/mol).

Consider the buffer pair, HF/F^-. What can be stated about the relative proportions of this buffer pair if the pH of an aqueous solution of this pair is adjusted tO₄.00 and the p K _a for HF equals 3.17?

A 20.0 mL sample of lactic acid (monoprotic with K _a = 1.37×10^{- 4}) requires 30.0 mL of 0.200 M NaOH for titration to the equivalence point. What is the concentration of the lactic acid solution?

Which of the following titration curves listed below best represents a curve for the complete titration of oxalic acid, H₂C₂O₄ (a diprotic acid), with a strong base such as NaOH?

A 350 mL volume of 0.150 M Ba(OH)₂ was completely neutralized by 35.0 mL of HCl. What is the molarity of the HCl solution?

A buffer is made by dissolving 0.10 mol of NaF in 1.00 L of 0.20 M HF. What is the pH of this buffer? K _a(HF) = 6.3×10^{- 4}

Which of the following titration curves listed below best represents a curve for the complete titration of the weakly basic dianion, sulfide, S^{2 -}, with a strong acid such as HCl as shown below in the net ionic equation? S^{2 -} (aq) + 2 HCl (aq)→H₂S (g) + 2 Cl^-

Calculate the number of moles of sodium acetate (CH₃COONa) that must be added to 1.00 L of 0.100 M CH₃COOH ( K _a = 1.8×10^{- 5}) to give a buffer with pH₅.00.

Calculate the pH of a solution after 10.0 mL of 0.100 M NaOH is added tO₄0.0 mL of 0.250 M HBr.

What is the pH of a buffer solution that consists of 0.25 M HClO₂ and 0.75 M KClO₂? K _a(HClO₂) = 1.1×10^{- 2}

Which pair(s) of substances would make a suitable buffer pair ? I. HCl and NaCl II. HF and NaF III. NH₄Cl and NH₃

What is the pH of a solution prepared by mixing 0.250 mol of hydrazoic acid, HN₃, and 0.500 mol of sodium azide, NaN₃, to make 1.00 liter of solution? ( K _a = 1.9×10^{- 5})