How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (Ka = 1.8 F1F1F1S1F1F1F10 10-5)? (Assume the volumes are additive.)

A) 30 mL B) 3 L C) 30 L D) 300 L E) 300 mL A) 30 mL B) 3 L C) 30 L D) 300 L E) 300 mL

Calculate the pH of a 2.0 F1F1F1S1F1F1F10 10-5 M solution of HOC6H5. (Ka = 1.6 F1F1F1S1F1F1F10 10-10)

A) 6.94 B) 6.75 C) 7.06 D) 7.25 E) none of these A) 6.94 B) 6.75 C) 7.06 D) 7.25 E) none of these

Calculate the pOH of a 0.70 M solution of acetic acid (Ka = 1.8 F1F1F1S1F1F1F10 10-5) at 25°C.

A) 2.72 B) 9.26 C) 4.90 D) 11.55 E) 2.45 A) 2.72 B) 9.26 C) 4.90 D) 11.55 E) 2.45

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO2, a weak acid), the equilibrium constant expression is

A) B) C) D) K = [H+][NO2-] E) none of these A) B) C) D) K = [H+][NO2-] E) none of these

HOAc Ka = 1.8 F1F1F1S1F1F1F1010-5 H2CO3 Ka1 = 4.3 F1F1F1S1F1F1F10 10-7, Ka2 = 5.6 F1F1F1S1F1F1F10 10-11 Which of the following 0.01 M solutions has the highest pH?

A) HOAc B) NaHCO3 C) H2CO3 D) NaOAc E) Na2CO3 A) HOAc B) NaHCO3 C) H2CO3 D) NaOAc E) Na2CO3

Calculate the pH of a 0.040 M perchloric acid (HClO4) solution.

A) 1.40 B) 2.10 C) 12.60 D) 11.90 E) none of these A) 1.40 B) 2.10 C) 12.60 D) 11.90 E) none of these

Calculate [H+] in a 0.012 M solution of HCN, Ka = 6.2 F1F1F1S1F1F1F10 10-10.

A) 3.0 F1F1F1S1F1F1F10 10-7 M B) 3.7 F1F1F1S1F1F1F10 10-9 M C) 6.2 F1F1F1S1F1F1F10 10-10 M D) 2.7 F1F1F1S1F1F1F10 10-6 M E) 2.3 F1F1F1S1F1F1F10 10-4 M A) 3.0 F1F1F1S1F1F1F10 10-7 M B) 3.7 F1F1F1S1F1F1F10 10-9 M C) 6.2 F1F1F1S1F1F1F10 10-10 M D) 2.7 F1F1F1S1F1F1F10 10-6 M E) 2.3 F1F1F1S1F1F1F10 10-4 M

Calculate [H+] in a 1.2 F1F1F1S1F1F1F10 10-5 M solution of NH4Cl. (Kb for NH3 = 1.8 F1F1F1S1F1F1F10 10-5)

A) 1.5 F1F1F1S1F1F1F10 10-5 M B) 8.2 F1F1F1S1F1F1F10 10-8 M C) 1.3 F1F1F1S1F1F1F10 10-7 M D) 1.2 F1F1F1S1F1F1F10 10-5 M E) 7.7 F1F1F1S1F1F1F10 10-8 M A) 1.5 F1F1F1S1F1F1F10 10-5 M B) 8.2 F1F1F1S1F1F1F10 10-8 M C) 1.3 F1F1F1S1F1F1F10 10-7 M D) 1.2 F1F1F1S1F1F1F10 10-5 M E) 7.7 F1F1F1S1F1F1F10 10-8 M

The following three equations represent equilibria that lie far to the right. HNOS1U1B13S1U1B0(aq) + CNS1U1P1-S1S1P0(aq) HCN(aq) + NOS1U1B13S1U1B0S1U1P1-S1S1P0(aq) HCN(aq) + OHS1U1P1-S1S1P0(aq) HS1U1B12S1U1B0O(l) + CNS1U1P1-S1S1P0(aq) HS1U1B12S1U1B0O(l) + CHS1U1B13S1U1B0OS1U1P1-S1S1P0(aq) CHS1U1B13S1U1B0OH(aq) + OHS1U1P1-S1S1P0(aq) -Identify the strongest base.

A) CH3OH B) CH3O- C) H2O D) NO3- E) CN- A) CH3OH B) CH3O- C) H2O D) NO3- E) CN-

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC2H3O2, C5H5NHCl, KOH, HCN. (Ka for HCN is 6.2 F1F1F1S1F1F1F10 10-10; Ka for HF is 7.2 F1F1F1S1F1F1F10 10-4; Ka for HC2H3O2 is 1.8 F1F1F1S1F1F1F10 10-5; and Kb for C5H5N is 1.7 F1F1F1S1F1F1F10 10-9)

A) C5H5NHCl, HCN, NaF, NaC2H3O2, KOH B) NaF, NaC2H3O2, HCN, C5H5NHCl, KOH C) KOH, NaC2H3O2, NaF, HCN, C5H5NHCl D) HCN, C5H5NHCl, NaF, NaC2H3O2, KOH E) none of these A) C5H5NHCl, HCN, NaF, NaC2H3O2, KOH B) NaF, NaC2H3O2, HCN, C5H5NHCl, KOH C) KOH, NaC2H3O2, NaF, HCN, C5H5NHCl D) HCN, C5H5NHCl, NaF, NaC2H3O2, KOH E) none of these

Exam 7: Acids and Bases

The pH of a strong acid solution is always lower than the pH of a weak acid solution. If this is true, explain why and include an example with calculations. If it is false, explain why and include a counterexample with calculations.

(True/False)

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Question 101

The pH of a solution made of 0.100 mol of a weak monoprotic acid HA in 1.000 L of solution is 1.470. Calculate K_a for this acid.

(Multiple Choice)

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Question 102

Calculate the pH of a 0.005 M solution of potassium oxide, K₂O.

(Multiple Choice)

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Question 103

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO₃)

(Multiple Choice)

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Question 104

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH4F) For NH₃, K_b = 1.8  10^-⁵; for HF, K_a = 7.2  10^-⁴.

(Multiple Choice)

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Question 105

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (K_a = 1.8  10^-⁵)? (Assume the volumes are additive.)

(Multiple Choice)

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Question 106

Calculate the pH of a 2.0  10^-⁵ M solution of HOC₆H₅. (K_a = 1.6  10^-¹⁰)

(Multiple Choice)

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Question 107

Calculate the pOH of a 0.70 M solution of acetic acid (K_a = 1.8  10^-⁵) at 25°C.

(Multiple Choice)

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Question 108

Which of the following reactions is associated with the definition of K_a?

(Multiple Choice)

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Question 109

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO₂, a weak acid), the equilibrium constant expression is

(Multiple Choice)

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Question 110

HOAc K_a = 1.8 10^-⁵ H₂CO₃K_a1 = 4.3  10^-⁷,K_a2 = 5.6  10^-¹¹ Which of the following 0.01 M solutions has the highest pH?

(Multiple Choice)

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Question 111

Calculate the pH of a 0.040 M perchloric acid (HClO₄) solution.

(Multiple Choice)

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Question 112

Calculate [H⁺] in a 0.012 M solution of HCN, K_a = 6.2  10^-¹⁰.

(Multiple Choice)

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Question 113

Which of the following species is not amphoteric?

(Multiple Choice)

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Question 114

The conjugate base of a weak acid is

(Multiple Choice)

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Question 115

Calculate [H⁺] in a 1.2  10^-⁵ M solution of NH₄Cl. (K_b for NH₃ = 1.8  10^-⁵)

(Multiple Choice)

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Question 116

The following three equations represent equilibria that lie far to the right. HNO₃(aq) + CN^-(aq) HCN(aq) + NO₃^-(aq) HCN(aq) + OH^-(aq) H₂O(l) + CN^-(aq) H₂O(l) + CH₃O^-(aq) CH₃OH(aq) + OH^-(aq) -Identify the strongest base.

(Multiple Choice)

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Question 117

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC₂H₃O₂, C₅H₅NHCl, KOH, HCN. (K_a for HCN is 6.2  10^-¹⁰; K_a for HF is 7.2  10^-⁴; K_a for HC₂H₃O₂ is 1.8  10^-⁵; and K_b for C₅H₅N is 1.7  10^-⁹)

(Multiple Choice)

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Question 118

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium cyanide (NaCN)

(Multiple Choice)

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Question 119

Showing 101 - 119 of 119

The pH of a strong acid solution is always lower than the pH of a weak acid solution. If this is true, explain why and include an example with calculations. If it is false, explain why and include a counterexample with calculations.

The pH of a solution made of 0.100 mol of a weak monoprotic acid HA in 1.000 L of solution is 1.470. Calculate K_a for this acid.

Calculate the pH of a 0.005 M solution of potassium oxide, K₂O.

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO₃)

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH4F) For NH₃, K_b = 1.8  10^-⁵; for HF, K_a = 7.2  10^-⁴.

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (K_a = 1.8  10^-⁵)? (Assume the volumes are additive.)

Calculate the pH of a 2.0  10^-⁵ M solution of HOC₆H₅. (K_a = 1.6  10^-¹⁰)

Calculate the pOH of a 0.70 M solution of acetic acid (K_a = 1.8  10^-⁵) at 25°C.

Which of the following reactions is associated with the definition of K_a?

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO₂, a weak acid), the equilibrium constant expression is

HOAc K_a = 1.8 10^-⁵ H₂CO₃K_a1 = 4.3  10^-⁷,K_a2 = 5.6  10^-¹¹ Which of the following 0.01 M solutions has the highest pH?

Calculate the pH of a 0.040 M perchloric acid (HClO₄) solution.

Calculate [H⁺] in a 0.012 M solution of HCN, K_a = 6.2  10^-¹⁰.

Which of the following species is not amphoteric?

The conjugate base of a weak acid is

Calculate [H⁺] in a 1.2  10^-⁵ M solution of NH₄Cl. (K_b for NH₃ = 1.8  10^-⁵)

The following three equations represent equilibria that lie far to the right. HNO₃(aq) + CN^-(aq) HCN(aq) + NO₃^-(aq) HCN(aq) + OH^-(aq) H₂O(l) + CN^-(aq) H₂O(l) + CH₃O^-(aq) CH₃OH(aq) + OH^-(aq) -Identify the strongest base.

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC₂H₃O₂, C₅H₅NHCl, KOH, HCN. (K_a for HCN is 6.2  10^-¹⁰; K_a for HF is 7.2  10^-⁴; K_a for HC₂H₃O₂ is 1.8  10^-⁵; and K_b for C₅H₅N is 1.7  10^-⁹)

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium cyanide (NaCN)

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Exam 7: Acids and Bases

The pH of a strong acid solution is always lower than the pH of a weak acid solution. If this is true, explain why and include an example with calculations. If it is false, explain why and include a counterexample with calculations.

The pH of a solution made of 0.100 mol of a weak monoprotic acid HA in 1.000 L of solution is 1.470. Calculate Ka for this acid.

Calculate the pH of a 0.005 M solution of potassium oxide, K2O.

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO3)

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH4F) For NH3, Kb = 1.8  10-5; for HF, Ka = 7.2  10-4.

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (Ka = 1.8  10-5)? (Assume the volumes are additive.)

Calculate the pH of a 2.0  10-5 M solution of HOC6H5. (Ka = 1.6  10-10)

Calculate the pOH of a 0.70 M solution of acetic acid (Ka = 1.8  10-5) at 25°C.

Which of the following reactions is associated with the definition of Ka?

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO2, a weak acid), the equilibrium constant expression is

HOAc Ka = 1.8 10-5 H2CO3 Ka1 = 4.3  10-7, Ka2 = 5.6  10-11 Which of the following 0.01 M solutions has the highest pH?

Calculate the pH of a 0.040 M perchloric acid (HClO4) solution.

Calculate [H+] in a 0.012 M solution of HCN, Ka = 6.2  10-10.

Which of the following species is not amphoteric?

The conjugate base of a weak acid is

Calculate [H+] in a 1.2  10-5 M solution of NH4Cl. (Kb for NH3 = 1.8  10-5)

The following three equations represent equilibria that lie far to the right. HNO3(aq) + CN-(aq) HCN(aq) + NO3-(aq) HCN(aq) + OH-(aq) H2O(l) + CN-(aq) H2O(l) + CH3O-(aq) CH3OH(aq) + OH-(aq) -Identify the strongest base.

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC2H3O2, C5H5NHCl, KOH, HCN. (Ka for HCN is 6.2  10-10; Ka for HF is 7.2  10-4; Ka for HC2H3O2 is 1.8  10-5; and Kb for C5H5N is 1.7  10-9)

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium cyanide (NaCN)

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Bonding: General Concepts

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The pH of a solution made of 0.100 mol of a weak monoprotic acid HA in 1.000 L of solution is 1.470. Calculate K_a for this acid.

Calculate the pH of a 0.005 M solution of potassium oxide, K₂O.

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO₃)

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH4F) For NH₃, K_b = 1.8  10^-⁵; for HF, K_a = 7.2  10^-⁴.

How much water should be added to 10.0 mL of 12.0 M HCl so that it has the same pH as 0.90 M acetic acid (K_a = 1.8  10^-⁵)? (Assume the volumes are additive.)

Calculate the pH of a 2.0  10^-⁵ M solution of HOC₆H₅. (K_a = 1.6  10^-¹⁰)

Calculate the pOH of a 0.70 M solution of acetic acid (K_a = 1.8  10^-⁵) at 25°C.

Which of the following reactions is associated with the definition of K_a?

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO₂, a weak acid), the equilibrium constant expression is

HOAc K_a = 1.8 10^-⁵ H₂CO₃K_a1 = 4.3  10^-⁷,K_a2 = 5.6  10^-¹¹ Which of the following 0.01 M solutions has the highest pH?

Calculate the pH of a 0.040 M perchloric acid (HClO₄) solution.

Calculate [H⁺] in a 0.012 M solution of HCN, K_a = 6.2  10^-¹⁰.

Calculate [H⁺] in a 1.2  10^-⁵ M solution of NH₄Cl. (K_b for NH₃ = 1.8  10^-⁵)

The following three equations represent equilibria that lie far to the right. HNO₃(aq) + CN^-(aq) HCN(aq) + NO₃^-(aq) HCN(aq) + OH^-(aq) H₂O(l) + CN^-(aq) H₂O(l) + CH₃O^-(aq) CH₃OH(aq) + OH^-(aq) -Identify the strongest base.

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC₂H₃O₂, C₅H₅NHCl, KOH, HCN. (K_a for HCN is 6.2  10^-¹⁰; K_a for HF is 7.2  10^-⁴; K_a for HC₂H₃O₂ is 1.8  10^-⁵; and K_b for C₅H₅N is 1.7  10^-⁹)