What is the equilibrium pH of a 0.700 M solution of H3PO4(aq)? (Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, Ka3 = 4.8 × 10-13)

A) 1.16 B) 3.68 C) 12.32 D) 6.24 E) 7.21 A) 1.16 B) 3.68 C) 12.32 D) 6.24 E) 7.21 A

What is the conjugate base of HPO43- in aqueous solution?

A) not possible B) PO43- C) HPO42− D) H2PO4− E) H3PO4 A) not possible B) PO43- C) HPO42− D) H2PO4− E) H3PO4

Which is the stronger Brønsted-Lowry acid, Fe(H2O)62+ or Fe(H2O)63+? Explain.

Fe(H 2 O) 6 3+ . When a proton dissociates from t

Rank H3PO4, H2PO4-, and HPO42- in order of increasing acid strength.

A) HPO42- 2PO4- 3PO4 B) H2PO4- 42- 3PO4 C) H2PO4- 3PO4 42- D) HPO42- 3PO4 2PO4- E) H3PO4 2PO4- 42- A) HPO42- 2PO4- 3PO4 B) H2PO4- 42- 3PO4 C) H2PO4- 3PO4 42- D) HPO42- 3PO4 2PO4- E) H3PO4 2PO4- 42-

Given the equilibrium constants for the equilibria, H2O(l) $\rightleftharpoons$ H3O+(aq); K = $5.69 \times 10 ^ { - 10 }$ 2CH3COOH(aq) + 2H2O(l) $\rightleftharpoons$ 2CH3COO?(aq) + 2H3O+(aq); K = $3.06 \times 10 ^ { - 10 }$ determine Kc for the following equilibrium. CH3COOH(aq) + NH3(aq) $\rightleftharpoons$ CH3COO?(aq) + NH4+(aq)

A) 3.08 × 104 B) 3.25 × 10-5 C) 9.96 × 10-15 D) 1.00 × 1014 E) 1.75 × 10-5 A) 3.08 × 104 B) 3.25 × 10-5 C) 9.96 × 10-15 D) 1.00 × 1014 E) 1.75 × 10-5

What is the pH of a 0.046 M HClO4(aq) at 25 °C? (Kw = 1.01 × 10-14)

A) 15.34 B) 3.08 C) 12.66 D) 1.34 E) 10.92 A) 15.34 B) 3.08 C) 12.66 D) 1.34 E) 10.92

Exam 17: Principles of Chemical Reactivity: the Chemistry of Acids and Bases

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What is the equilibrium pH of a 0.700 M solution of H₃PO₄(aq)? (K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, K_a3 = 4.8 × 10^-13)

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Question 1

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Which of the following is the correct equation for the reaction of ammonia in water?

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Question 2

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Which of the following ionic compounds forms a neutral aqueous solution at 25 °C?

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Question 3

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Given the following acid dissociation constants: K_a (H₃PO₄) = 7.5 × 10^-3 K_a (NH₄⁺) = 5.6 × 10^-10 Determine the equilibrium constant for the reaction below at 25 °C. H₃PO₄(aq) + NH₃(aq) $\rightleftharpoons$ NH₄⁺(aq) + H₂PO₄?(aq)

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Question 4

What is the pH of a solution prepared by dissolving 0.523 g of NaOH(s) in 5.50 L of water? (K_w = 1.01 × 10^-14)

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Question 5

What is the hydronium-ion concentration in a solution formed by combining 750 mL of 0.10 M NaOH with 250 mL of 0.30 M HCl? NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l)

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Question 6

Which of the following statements is true of the acid-base properties of common cations and anions in aqueous solutions?

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Question 7

What is the pH of the final solution when 25 mL of 0.021 M HCl has been added to 35 mL of 0.035 M HCl at 25°C?

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Question 8

Which of the following is the strongest acid in aqueous solution?

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Question 9

Which equation depicts aqueous hydrogen sulfide behaving as a Brønsted-Lowry base in water?

(Multiple Choice)

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Question 10

What is the pOH of 0.074 M HI(aq) at 25 °C? (K_w = 1.01 × 10^-14)?

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Question 11

What is the conjugate base of HPO₄^3- in aqueous solution?

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Question 12

What is the pH of 0.010 M aqueous hypochlorous acid? (K_a of HOCl = 3.5 × 10^-8)

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Question 13

Which of the following statements is INCORRECT?

(Multiple Choice)

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Question 14

Which is the stronger Brønsted-Lowry acid, Fe(H₂O)₆²⁺ or Fe(H₂O)₆³⁺? Explain.

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Question 15

All of the following compounds are acids containing chlorine. Which compound is the weakest acid?

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Question 16

Rank H₃PO₄, H₂PO₄^-, and HPO₄^2- in order of increasing acid strength.

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Question 17

Given the equilibrium constants for the equilibria, H₂O(l) $\rightleftharpoons$ H₃O⁺(aq); K = $5.69 \times 10 ^ { - 10 }$ 2CH₃COOH(aq) + 2H₂O(l) $\rightleftharpoons$ 2CH₃COO?(aq) + 2H₃O⁺(aq); K = $3.06 \times 10 ^ { - 10 }$ determine K_c for the following equilibrium. CH₃COOH(aq) + NH₃(aq) $\rightleftharpoons$ CH₃COO?(aq) + NH₄⁺(aq)

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Question 18

Which one of the following aqueous solutions will have a pH of 2.00 at 25 °C? (K_w = 1.01 × 10^-14)

(Multiple Choice)

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Question 19

What is the pH of a 0.046 M HClO₄(aq) at 25 °C? (K_w = 1.01 × 10^-14)

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Question 20

Showing 1 - 20 of 97

Exam 17: Principles of Chemical Reactivity: the Chemistry of Acids and Bases

What is the equilibrium pH of a 0.700 M solution of H3PO4(aq)? (Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, Ka3 = 4.8 × 10-13)

Which of the following is the correct equation for the reaction of ammonia in water?

Which of the following ionic compounds forms a neutral aqueous solution at 25 °C?

Given the following acid dissociation constants: Ka (H3PO4) = 7.5 × 10-3 Ka (NH4+) = 5.6 × 10-10 Determine the equilibrium constant for the reaction below at 25 °C. H3PO4(aq) + NH3(aq) ⇌\rightleftharpoons⇌ NH4+(aq) + H2PO4?(aq)

What is the pH of a solution prepared by dissolving 0.523 g of NaOH(s) in 5.50 L of water? (Kw = 1.01 × 10-14)

What is the hydronium-ion concentration in a solution formed by combining 750 mL of 0.10 M NaOH with 250 mL of 0.30 M HCl? NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)

Which of the following statements is true of the acid-base properties of common cations and anions in aqueous solutions?

What is the pH of the final solution when 25 mL of 0.021 M HCl has been added to 35 mL of 0.035 M HCl at 25°C?

Which of the following is the strongest acid in aqueous solution?

Which equation depicts aqueous hydrogen sulfide behaving as a Brønsted-Lowry base in water?

What is the pOH of 0.074 M HI(aq) at 25 °C? (Kw = 1.01 × 10-14)?

What is the conjugate base of HPO43- in aqueous solution?

What is the pH of 0.010 M aqueous hypochlorous acid? (Ka of HOCl = 3.5 × 10-8)

Which of the following statements is INCORRECT?

Which is the stronger Brønsted-Lowry acid, Fe(H2O)62+ or Fe(H2O)63+? Explain.

All of the following compounds are acids containing chlorine. Which compound is the weakest acid?

Rank H3PO4, H2PO4-, and HPO42- in order of increasing acid strength.

Which one of the following aqueous solutions will have a pH of 2.00 at 25 °C? (Kw = 1.01 × 10-14)

What is the pH of a 0.046 M HClO4(aq) at 25 °C? (Kw = 1.01 × 10-14)

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

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Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

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What is the equilibrium pH of a 0.700 M solution of H₃PO₄(aq)? (K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, K_a3 = 4.8 × 10^-13)

Given the following acid dissociation constants: K_a (H₃PO₄) = 7.5 × 10^-3 K_a (NH₄⁺) = 5.6 × 10^-10 Determine the equilibrium constant for the reaction below at 25 °C. H₃PO₄(aq) + NH₃(aq) $\rightleftharpoons$ NH₄⁺(aq) + H₂PO₄?(aq)

What is the pH of a solution prepared by dissolving 0.523 g of NaOH(s) in 5.50 L of water? (K_w = 1.01 × 10^-14)

What is the hydronium-ion concentration in a solution formed by combining 750 mL of 0.10 M NaOH with 250 mL of 0.30 M HCl? NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l)

What is the pOH of 0.074 M HI(aq) at 25 °C? (K_w = 1.01 × 10^-14)?

What is the conjugate base of HPO₄^3- in aqueous solution?

What is the pH of 0.010 M aqueous hypochlorous acid? (K_a of HOCl = 3.5 × 10^-8)

Which is the stronger Brønsted-Lowry acid, Fe(H₂O)₆²⁺ or Fe(H₂O)₆³⁺? Explain.

Rank H₃PO₄, H₂PO₄^-, and HPO₄^2- in order of increasing acid strength.

Which one of the following aqueous solutions will have a pH of 2.00 at 25 °C? (K_w = 1.01 × 10^-14)

What is the pH of a 0.046 M HClO₄(aq) at 25 °C? (K_w = 1.01 × 10^-14)