A solution with a hydrogen ion concentration of 3.25 × 10-5 M is ________ and has a hydroxide ion concentration of ________.

A) acidic, 3.08 × 10-9 M B) acidic, 3.08 × 10-10 M C) basic, 3.08 × 10-9 M D) basic, 3.08 × 10-10 M A) acidic, 3.08 × 10-9 M B) acidic, 3.08 × 10-10 M C) basic, 3.08 × 10-9 M D) basic, 3.08 × 10-10 M

Determine the pH of a solution that is 0.15 M HClO2 (Ka = 1.1 × 10-2)and 0.15 M HClO (Ka = 2.9 × 10-8).

A) 4.18 B) 9.82 C) 12.55 D) 1.39 E) 3.55 A) 4.18 B) 9.82 C) 12.55 D) 1.39 E) 3.55

Calculate the pOH of a solution that contains 3.9 × 10-4 M H3O⁺ at 25°C.

A) 4.41 B) 3.41 C) 10.59 D) 9.59 E) 0.59 A) 4.41 B) 3.41 C) 10.59 D) 9.59 E) 0.59

Determine the Ka for CH3NH3⁺ at 25°C.The Kb for CH3NH2 is 4.4 × 10-4.

A) 3.1 × 10-10 B) 6.8 × 10-11 C) 5.6 × 10-10 D) 2.3 × 10-3 E) 2.3 × 10-11 A) 3.1 × 10-10 B) 6.8 × 10-11 C) 5.6 × 10-10 D) 2.3 × 10-3 E) 2.3 × 10-11

What is the pH of a 0.020 M HClO4 solution?

A) 0.020 B) 0.040 C) 1.70 D) 12.30 A) 0.020 B) 0.040 C) 1.70 D) 12.30

Determine the pH of a 0.232 M Ca(OH)2 solution at 25°C.

A) 12.73 B) 13.37 C) 13.67 D) 0.333 E) 0.634 A) 12.73 B) 13.37 C) 13.67 D) 0.333 E) 0.634

The base-dissociation constant of ethylamine (C2H5NH2)is 6.4 × 10-4 at 25.0°C.The [H+] in a solution of ethylamine is ________ M.

A) 3.5 × 10-12 B) 2.9 × 10-3 C) 3.1 × 10-12 D) 3.2 × 10-3 E) 11.46 A) 3.5 × 10-12 B) 2.9 × 10-3 C) 3.1 × 10-12 D) 3.2 × 10-3 E) 11.46

Calculate the pH of a 0.80 M H2SO3,solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and

A) 0.96 B) 0.99 C) 1.82 D) 1.92 A) 0.96 B) 0.99 C) 1.82 D) 1.92

Determine the pOH of a 0.00598 M HClO4 solution.

A) 11.777 B) 6.434 C) 7.566 D) 2.223 E) 3.558 A) 11.777 B) 6.434 C) 7.566 D) 2.223 E) 3.558

Exam 17: Acids and Bases

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What is the pH of a 1.2 M pyridine solution that has K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is C₅H₅N(aq)+ H₂O(l)⇌ C₅H₅NH⁺(aq)+ OH^-(aq).

(Multiple Choice)

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Question 101

A solution with a hydrogen ion concentration of 3.25 × 10^-⁵ M is and has a hydroxide ion concentration of .

(Multiple Choice)

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Question 102

Which of the following species is amphoteric?

(Multiple Choice)

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Question 103

Calculate the pH for an aqueous solution of pyridine that contains hydroxide ion.

(Multiple Choice)

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Question 104

Calculate the hydroxide ion concentration in an aqueous solution with a pOH of 9.85 at 25°C.

(Multiple Choice)

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Question 105

Determine the pH of a solution that is 0.15 M HClO₂ (K_a = 1.1 × 10^-2)and 0.15 M HClO (K_a = 2.9 × 10^-8).

(Multiple Choice)

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Question 106

Calculate the pOH of a solution that contains 3.9 × 10^-⁴ M H₃O⁺ at 25°C.

(Multiple Choice)

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Question 107

Determine the K_a for CH₃NH₃⁺ at 25°C.The K_b for CH₃NH₂ is 4.4 × 10^-4.

(Multiple Choice)

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Question 108

Which of the following weak acids has the strongest conjugate base?

(Multiple Choice)

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Question 109

What is the pH of a 0.020 M HClO₄ solution?

(Multiple Choice)

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Question 110

Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25^∘C.The acid is followed by its K_a value.

(Multiple Choice)

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Question 111

Which of the following is a weak acid?

(Multiple Choice)

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Question 112

Determine the K_a of an acid that has a pH of 3.29 and a concentration of 0.55 M.

(Multiple Choice)

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Question 113

Determine the pH of a 0.232 M Ca(OH)₂ solution at 25°C.

(Multiple Choice)

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Question 114

When dissolved in water,which compound is generally considered to be an Arrhenius acid?

(Multiple Choice)

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Question 115

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C.

(Multiple Choice)

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Question 116

The base-dissociation constant of ethylamine (C₂H₅NH₂)is 6.4 × 10^-4 at 25.0°C.The [H⁺] in a solution of ethylamine is ________ M.

(Multiple Choice)

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Question 117

Calculate the pH of a 0.80 M H₂SO₃,solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and

(Multiple Choice)

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Question 118

Determine the pOH of a 0.00598 M HClO₄ solution.

(Multiple Choice)

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Question 119

Identify the food that is not acidic.

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Question 120

Showing 101 - 120 of 159

Exam 17: Acids and Bases

What is the pH of a 1.2 M pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is C5H5N(aq)+ H2O(l)⇌ C5H5NH+(aq)+ OH-(aq).

A solution with a hydrogen ion concentration of 3.25 × 10-5 M is ________ and has a hydroxide ion concentration of ________.

Which of the following species is amphoteric?

Calculate the pH for an aqueous solution of pyridine that contains hydroxide ion.

Calculate the hydroxide ion concentration in an aqueous solution with a pOH of 9.85 at 25°C.

Determine the pH of a solution that is 0.15 M HClO2 (Ka = 1.1 × 10-2)and 0.15 M HClO (Ka = 2.9 × 10-8).

Calculate the pOH of a solution that contains 3.9 × 10-4 M H3O⁺ at 25°C.

Determine the Ka for CH3NH3⁺ at 25°C.The Kb for CH3NH2 is 4.4 × 10-4.

Which of the following weak acids has the strongest conjugate base?

What is the pH of a 0.020 M HClO4 solution?

Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25∘C.The acid is followed by its Ka value.

Which of the following is a weak acid?

Determine the Ka of an acid that has a pH of 3.29 and a concentration of 0.55 M.

Determine the pH of a 0.232 M Ca(OH)2 solution at 25°C.

When dissolved in water,which compound is generally considered to be an Arrhenius acid?

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C.

The base-dissociation constant of ethylamine (C2H5NH2)is 6.4 × 10-4 at 25.0°C.The [H+] in a solution of ethylamine is ________ M.

Calculate the pH of a 0.80 M H2SO3,solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and

Determine the pOH of a 0.00598 M HClO4 solution.

Identify the food that is not acidic.

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What is the pH of a 1.2 M pyridine solution that has K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is C₅H₅N(aq)+ H₂O(l)⇌ C₅H₅NH⁺(aq)+ OH^-(aq).

A solution with a hydrogen ion concentration of 3.25 × 10^-⁵ M is and has a hydroxide ion concentration of .

Determine the pH of a solution that is 0.15 M HClO₂ (K_a = 1.1 × 10^-2)and 0.15 M HClO (K_a = 2.9 × 10^-8).

Calculate the pOH of a solution that contains 3.9 × 10^-⁴ M H₃O⁺ at 25°C.

Determine the K_a for CH₃NH₃⁺ at 25°C.The K_b for CH₃NH₂ is 4.4 × 10^-4.

What is the pH of a 0.020 M HClO₄ solution?

Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25^∘C.The acid is followed by its K_a value.

Determine the K_a of an acid that has a pH of 3.29 and a concentration of 0.55 M.

Determine the pH of a 0.232 M Ca(OH)₂ solution at 25°C.

The base-dissociation constant of ethylamine (C₂H₅NH₂)is 6.4 × 10^-4 at 25.0°C.The [H⁺] in a solution of ethylamine is ________ M.

Calculate the pH of a 0.80 M H₂SO₃,solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and

Determine the pOH of a 0.00598 M HClO₄ solution.