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 acid.

A) HNO3 B) HCN C) OH- D) H2O E) CH3OH A) HNO3 B) HCN C) OH- D) H2O E) CH3OH

The dihydrogenphosphate ion, H2PO4-, has both a conjugate acid and a conjugate base. These are, respectively,

A) H2PO4- and HPO42- B) HPO42- and H3PO4 C) HPO42- and PO43- D) H3PO4 and PO43- E) H3PO4 and HPO42- A) H2PO4- and HPO42- B) HPO42- and H3PO4 C) HPO42- and PO43- D) H3PO4 and PO43- E) H3PO4 and HPO42-

Calculate the [H+] in a 2.0 F1F1F1S1F1F1F10 10-6 M solution of NaC2H3O2.(Ka for HC2H3O2 = 1.8 F1F1F1S1F1F1F10 10-5)

A) 6.0 F1F1F1S1F1F1F10 10-6 M B) 1.7 F1F1F1S1F1F1F10 10-9 M C) 3.4 F1F1F1S1F1F1F10 10-8 M D) 1.1 F1F1F1S1F1F1F10 10-7 M E) 9.6 F1F1F1S1F1F1F10 10-8 M A) 6.0 F1F1F1S1F1F1F10 10-6 M B) 1.7 F1F1F1S1F1F1F10 10-9 M C) 3.4 F1F1F1S1F1F1F10 10-8 M D) 1.1 F1F1F1S1F1F1F10 10-7 M E) 9.6 F1F1F1S1F1F1F10 10-8 M

The conjugate acid and conjugate base of bicarbonate ion, HCO3-, are, respectively,

A) H3O+ and OH- B) H2CO3 and OH- C) H3O+ and CO32- D) H2CO3 and CO32- E) CO32- and OH- A) H3O+ and OH- B) H2CO3 and OH- C) H3O+ and CO32- D) H2CO3 and CO32- E) CO32- and OH-

How many moles of benzoic acid, a monoprotic acid with Ka = 6.4 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-5, must be dissolved in 500. mL of H2O to produce a solution with pH = 2.50?

A) 1.6 F1F1F1S1F1F1F10 10-1 B) 2.0 F1F1F1S1F1F1F10 10-2 C) 7.8 F1F1F1S1F1F1F10 10-2 D) 0.50 E) none of these A) 1.6 F1F1F1S1F1F1F10 10-1 B) 2.0 F1F1F1S1F1F1F10 10-2 C) 7.8 F1F1F1S1F1F1F10 10-2 D) 0.50 E) none of these

Determine the pH of a solution made by adding 1.0 * 10-7 mol of HCl to 1.0 L of solution.

The answer of Determine the pH of a solution made...

In pure liquid ammonia, the equilibrium concentrations of both NH4+ and NH2- are 3 F1F1F1S1F1F1F10 10-14 M. Which of the following equations always holds for liquid ammonia solutions?

A) pNH4+ = log [pNH4+] B) pNH4+ = 27.0 C) pNH4+ - pNH2- = 13.5 D) pNH4+ = 27.0 - pNH2- E) pNH4+ + pNH2- = 13.5 A) pNH4+ = log [pNH4+] B) pNH4+ = 27.0 C) pNH4+ - pNH2- = 13.5 D) pNH4+ = 27.0 - pNH2- E) pNH4+ + pNH2- = 13.5

Calculate [OH-] in a 4.0 F1F1F1S1F1F1F10 10-8 M solution of NaOH.

A) 8.2 F1F1F1S1F1F1F10 10-8 M B) 6.7 F1F1F1S1F1F1F10 10-6 M C) 2.5 F1F1F1S1F1F1F10 10-7 M D) 4.0 F1F1F1S1F1F1F10 10-8 M E) 1.2 F1F1F1S1F1F1F10 10-7 M A) 8.2 F1F1F1S1F1F1F10 10-8 M B) 6.7 F1F1F1S1F1F1F10 10-6 M C) 2.5 F1F1F1S1F1F1F10 10-7 M D) 4.0 F1F1F1S1F1F1F10 10-8 M E) 1.2 F1F1F1S1F1F1F10 10-7 M

Find the pH of a solution at 25°C in which [OH-] = 2.5 F1F1F1S1F1F1F10 10-9 M.

A) 6.50 B) 8.60 C) 7.40 D) 2.50 E) 5.40 A) 6.50 B) 8.60 C) 7.40 D) 2.50 E) 5.40

Exam 7: Acids and Bases

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 acid.

(Multiple Choice)

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Question 81

The dihydrogenphosphate ion, H₂PO₄^-, has both a conjugate acid and a conjugate base. These are, respectively,

(Multiple Choice)

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Question 82

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid potassium chloride (KCl)

(Multiple Choice)

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Question 83

Which of the following is a conjugate acid-base pair?

(Multiple Choice)

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Question 84

Identify the Brønsted acids and bases in the following equation (A = Brønsted acid, B = Brønsted base). HPO₄²^- + HSO₄^- H₂PO₄^- + SO₄²^-

(Multiple Choice)

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Question 85

Calculate the [H⁺] in a 2.0  10^-⁶ M solution of NaC₂H₃O₂.(K_a for HC₂H₃O₂ = 1.8  10^-⁵)

(Multiple Choice)

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Question 86

The conjugate acid and conjugate base of bicarbonate ion, HCO₃^-, are, respectively,

(Multiple Choice)

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Question 87

How many moles of benzoic acid, a monoprotic acid with K_a = 6.4 10^-⁵, must be dissolved in 500. mL of H₂O to produce a solution with pH = 2.50?

(Multiple Choice)

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Question 88

Which of the following statements is true for polyprotic acids?

(Multiple Choice)

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Question 89

The pH of a solution is raised from 3 to 5. Which statement is false?

(Multiple Choice)

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Question 90

The pH of a 0.013 M weak acid solution is 5.27. Calculate K_a for this acid.

(Multiple Choice)

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Question 91

Which of the following represents a conjugate acid-base pair?

(Multiple Choice)

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Question 92

The salt BX, when dissolved in water, produces an acidic solution. Which of the following could be true?

(Multiple Choice)

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Question 93

The pK_a of HOCl is 7.5. Calculate the pH of a 0.5 M solution of HOCl.

(Multiple Choice)

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Question 94

Calculate the pH of a solution made by mixing equal volumes of a solution of NaOH with a pH of 11.40 and a solution of KOH with a pH of 10.30. (Assume the volumes are additive.)

(Multiple Choice)

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Question 95

Determine the pH of a solution made by adding 1.0 * 10^-⁷ mol of HCl to 1.0 L of solution.

(Short Answer)

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Question 96

In pure liquid ammonia, the equilibrium concentrations of both NH₄⁺ and NH₂^- are 3  10^-¹⁴ M. Which of the following equations always holds for liquid ammonia solutions?

(Multiple Choice)

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Question 97

Calculate [OH^-] in a 4.0  10^-⁸ M solution of NaOH.

(Multiple Choice)

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Question 98

A 0.050 M aqueous solution of a weak monoprotic acid is 1.2% ionized at equilibrium at 25° C. Calculate K_a for this acid.

(Multiple Choice)

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Question 99

Find the pH of a solution at 25°C in which [OH^-] = 2.5  10^-⁹ M.

(Multiple Choice)

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Question 100

Showing 81 - 100 of 119

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 acid.

The dihydrogenphosphate ion, H₂PO₄^-, has both a conjugate acid and a conjugate base. These are, respectively,

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid potassium chloride (KCl)

Which of the following is a conjugate acid-base pair?

Identify the Brønsted acids and bases in the following equation (A = Brønsted acid, B = Brønsted base). HPO₄²^- + HSO₄^- H₂PO₄^- + SO₄²^-

Calculate the [H⁺] in a 2.0  10^-⁶ M solution of NaC₂H₃O₂.(K_a for HC₂H₃O₂ = 1.8  10^-⁵)

The conjugate acid and conjugate base of bicarbonate ion, HCO₃^-, are, respectively,

How many moles of benzoic acid, a monoprotic acid with K_a = 6.4 10^-⁵, must be dissolved in 500. mL of H₂O to produce a solution with pH = 2.50?

Which of the following statements is true for polyprotic acids?

The pH of a solution is raised from 3 to 5. Which statement is false?

The pH of a 0.013 M weak acid solution is 5.27. Calculate K_a for this acid.

Which of the following represents a conjugate acid-base pair?

The salt BX, when dissolved in water, produces an acidic solution. Which of the following could be true?

The pK_a of HOCl is 7.5. Calculate the pH of a 0.5 M solution of HOCl.

Calculate the pH of a solution made by mixing equal volumes of a solution of NaOH with a pH of 11.40 and a solution of KOH with a pH of 10.30. (Assume the volumes are additive.)

Determine the pH of a solution made by adding 1.0 * 10^-⁷ mol of HCl to 1.0 L of solution.

In pure liquid ammonia, the equilibrium concentrations of both NH₄⁺ and NH₂^- are 3  10^-¹⁴ M. Which of the following equations always holds for liquid ammonia solutions?

Calculate [OH^-] in a 4.0  10^-⁸ M solution of NaOH.

A 0.050 M aqueous solution of a weak monoprotic acid is 1.2% ionized at equilibrium at 25° C. Calculate K_a for this acid.

Find the pH of a solution at 25°C in which [OH^-] = 2.5  10^-⁹ M.

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Exam 7: Acids and Bases

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 acid.

The dihydrogenphosphate ion, H2PO4-, has both a conjugate acid and a conjugate base. These are, respectively,

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid potassium chloride (KCl)

Which of the following is a conjugate acid-base pair?

Identify the Brønsted acids and bases in the following equation (A = Brønsted acid, B = Brønsted base). HPO42- + HSO4- H2PO4- + SO42-

Calculate the [H+] in a 2.0  10-6 M solution of NaC2H3O2.(Ka for HC2H3O2 = 1.8  10-5)

The conjugate acid and conjugate base of bicarbonate ion, HCO3-, are, respectively,

How many moles of benzoic acid, a monoprotic acid with Ka = 6.4 10-5, must be dissolved in 500. mL of H2O to produce a solution with pH = 2.50?

Which of the following statements is true for polyprotic acids?

The pH of a solution is raised from 3 to 5. Which statement is false?

The pH of a 0.013 M weak acid solution is 5.27. Calculate Ka for this acid.

Which of the following represents a conjugate acid-base pair?

The salt BX, when dissolved in water, produces an acidic solution. Which of the following could be true?

The pKa of HOCl is 7.5. Calculate the pH of a 0.5 M solution of HOCl.

Calculate the pH of a solution made by mixing equal volumes of a solution of NaOH with a pH of 11.40 and a solution of KOH with a pH of 10.30. (Assume the volumes are additive.)

Determine the pH of a solution made by adding 1.0 * 10-7 mol of HCl to 1.0 L of solution.

In pure liquid ammonia, the equilibrium concentrations of both NH4+ and NH2- are 3  10-14 M. Which of the following equations always holds for liquid ammonia solutions?

Calculate [OH-] in a 4.0  10-8 M solution of NaOH.

A 0.050 M aqueous solution of a weak monoprotic acid is 1.2% ionized at equilibrium at 25° C. Calculate Ka for this acid.

Find the pH of a solution at 25°C in which [OH-] = 2.5  10-9 M.

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Chemical Equilibrium

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

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 acid.

The dihydrogenphosphate ion, H₂PO₄^-, has both a conjugate acid and a conjugate base. These are, respectively,

Identify the Brønsted acids and bases in the following equation (A = Brønsted acid, B = Brønsted base). HPO₄²^- + HSO₄^- H₂PO₄^- + SO₄²^-

Calculate the [H⁺] in a 2.0  10^-⁶ M solution of NaC₂H₃O₂.(K_a for HC₂H₃O₂ = 1.8  10^-⁵)

The conjugate acid and conjugate base of bicarbonate ion, HCO₃^-, are, respectively,

How many moles of benzoic acid, a monoprotic acid with K_a = 6.4 10^-⁵, must be dissolved in 500. mL of H₂O to produce a solution with pH = 2.50?

The pH of a 0.013 M weak acid solution is 5.27. Calculate K_a for this acid.

The pK_a of HOCl is 7.5. Calculate the pH of a 0.5 M solution of HOCl.

Determine the pH of a solution made by adding 1.0 * 10^-⁷ mol of HCl to 1.0 L of solution.

In pure liquid ammonia, the equilibrium concentrations of both NH₄⁺ and NH₂^- are 3  10^-¹⁴ M. Which of the following equations always holds for liquid ammonia solutions?

Calculate [OH^-] in a 4.0  10^-⁸ M solution of NaOH.

A 0.050 M aqueous solution of a weak monoprotic acid is 1.2% ionized at equilibrium at 25° C. Calculate K_a for this acid.

Find the pH of a solution at 25°C in which [OH^-] = 2.5  10^-⁹ M.