Which of the following statements is false? (a) An Arrhenius base increases the concentration of OH- in water. (b) A Brønsted-Lowry base is a proton acceptor. (c) Water can act as a Brønsted–Lowry acid. (d) Water can act as a Brønsted–Lowry base. (e) Any compound that contains an –OH group acts as a Brønsted-Lowry base.

Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+.

Give the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-.

Give the conjugate acid of the following Brønsted–Lowry bases: (i) SO42-, (ii) CH3NH2.

Identify the Brønsted–Lowry acid and the Brønsted–Lowry base on the left side of each of the following equations, and also identify the conjugate acid and conjugate base of each on the right side:

(a) NH₄⁺(aq) + CN^-(aq) ⇌ HCN(aq) + NH₃(aq)

(b) (CH₃)₃N(aq) + H₂O(l) ⇌ (CH₃)₃NH⁺(aq) + OH^-(aq)

(c) HCOOH(aq) + PO₄^3-(aq) ⇌ HCOO^-(aq)+ HPO₄^2-(aq)

Identify the Brønsted–Lowry acid and the Brønsted– Lowry base on the left side of each equation, and also identify the conjugate acid and conjugate base of each on the right side.

(a) HBrO(aq) + H₂O(l) ⇌ H₃O⁺(aq) + BrO^-(aq)

(b) HSO₄^-(aq) + HCO₃^-(aq) ⇌ SO₄^2-(aq) + H₂CO₃(aq)

(c) HSO₃^-(aq) + H₃O⁺(aq) ⇌ H₂SO₃(aq) + H₂O(l)

The hydrogen sulfite ion 1HSO3-2 is amphiprotic. Write a balanced chemical equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water.

What is the conjugate acid of HSO3-? What is its conjugate base?

Write an equation for the reaction in which H2C6H7O5-1aq2 acts as a base in H2O1l2.

Write an equation for the reaction in which H2C6H7O5-1aq2 acts as an acid in H2O1l2.

Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (a) CH3COO-

Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (b) HCO3-

Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (c) O2-

Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (d) Cl-

Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (e) NH3.

Which of the following is the stronger Brønsted–Lowry acid, HBrO or HBr?

Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow:

(a) O^2-(aq) + H₂O(l) ⇌

(b) CH₃COOH(aq) + HS^-(aq) ⇌

(c) NO₂^-(aq) + H₂O(l) ⇌

Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow:

(a) NH₄⁺(aq) + OH^-(aq) ⇌

(b) CH₃COO^-(aq) + H₃O⁺(aq) ⇌

(c) HCO₃^-(aq) + F^-(aq) ⇌

Write a chemical equation that illustrates the autoionization of water.

Write the expression for the ion product constant for water, K_w.

Calculate [H⁺] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) [OH^-] = 0.00045 M (b) [OH^-] = 8.8 × 10^-9 M (c) a solution in which [OH^-] is 100 times greater than [H⁺].

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) 3H+4 = 0.0505 M

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3H+4 = 2.5 * 10-10 M

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (c) a solution in which 3H+4 is 1000 times greater than 3OH-4.