Topic 8 Acids and Bases

What is the difference between a conjugate Brønsted–Lowry acid–base pair?

• Electron pair

• Positive charge

• Proton

• Hydrogen atom

Which is an example of an amphiprotic species?

• Al₂O₃

• CO₃²⁻

• P₄O₁₀

• HPO₄²⁻

Which two species act as Brønsted–Lowry acids in the reaction?

H₂PO₄⁻ (aq) + OH⁻ (aq) ⇌

HPO₄²⁻ (aq) + H₂O (l)

• HPO₄²⁻ (aq) and OH⁻ (aq)

• H₂PO₄⁻ (aq) and HPO₄²⁻ (aq)

• HPO₄²⁻ (aq) and H₂O (l)

• H₂PO₄⁻ (aq) and H₂O (l)

Which classification is correct for the reaction?

H₂PO₄⁻(aq) + H₂O(l) → HPO₄²⁻(aq) + H₃O⁺(aq)

• A

• B

• C

• D

What describes HPO₄²⁻?

• Amphiprotic but not amphoteric

• Amphoteric but not amphiprotic

• Amphiprotic and amphoteric

• Neither amphiprotic nor amphoteric

Which is an acid-base conjugate pair?

• H₃O⁺ / OH^–

• H₂SO₄ / SO₄^2–

• CH₃COOH / H₃O⁺

• CH₃NH₃⁺ / CH₃NH₂

Which of the following is correct?

• A weak acid is a proton donor and its aqueous solution shows good conductivity.

• A weak acid is a proton donor and its aqueous solution shows poor conductivity.

• A weak acid is a proton acceptor and its aqueous solution shows good conductivity.

• A weak acid is a proton acceptor and its aqueous solution shows poor conductivity.

Which species produced by the successive dissociations of phosphoric acid, H₃PO₄, are amphiprotic?

• HPO₄²⁻ and PO₄³⁻

• H₂PO₄⁻ and HPO₄²⁻

• H₂PO₄⁻ and PO₄³⁻

• HPO₄²⁻ only

Which species acts as a Lewis and Brønsted–Lowry base?

• [Al(H₂O)₆]³⁺

• BF₃

• NH₄⁺

• OH⁻

Which species behave as Brønsted–Lowry bases in the following reaction?

H₂SO₄ + HNO₃ H₂NO₃⁺ + HSO₄^-

• HNO₃ and HSO₄^-

• HNO₃ and H₂NO₃⁺

• H₂SO₄ and HSO₄^-

• H₂NO₃⁺ and HSO₄^-