Acids, Bases and pH - exam practice

Which are the Brønsted-Lowry acids in the following equilibrium?

CH₃COOH + C₂H₅COOH ⇌ CH₃COO^- + C₂H₅COOH₂⁺

A solution of hydrochloric acid has pH = 2.

The solution is diluted to one tenth of its original concentration.

What is the pH of the diluted solution?

Ammonia reacts with water in a reversible reaction. Which are the Brønsted-Lowry bases?

20 cm³ of 0.10 mol dm^-3 hydrochloric acid is added to 10 cm³ of 0.10 mol dm^-3 sodium hydroxide.

What is the pH of the resulting mixture?

The equation shows the dissociation of the acid H₃AsO₄ in water.

H3AsO₄ + H₂O ⇌ H₂AsO₄^- + H₃O⁺

Which pair is a conjugate acid–base pair?

2,4,6-Trichlorophenol is a weak monoprotic acid, with K_a = 2.51 × 10^-8 mol dm^-3 at 298 K.

What is the concentration, in mol dm^-3, of hydrogen ions in a 2.00 × 10^-3 mol dm^-3 solution of 2,4,6-trichlorophenol at 298 K?

What is the pH of a 0.46 mol dm^-3 solution of potassium hydroxide at 298 K?

K_w = 1.0 × 10^-14 mol² dm^-6 at 298 K.

The acid dissociation constant, K_a, of a weak acid HA has the value 2.56 × 10^-4 mol dm^-3

What is the pH of a 4.25 × 10^-3 mol dm^-3 solution of HA?

Which is the concentration of NaOH_(aq), in mol dm^-3, that has pH = 14.30?

K_w = 1.00 × 10^-14 mol² dm^-6 at 25°C

What is the pH of 0.015 mol dm^-3 sulfuric acid?

How are 20 cm³ of 0.05 mol dm^-3 H₂SO_4(aq) and 20 cm³ of 0.10 mol dm^-3 CH₃COOH_(aq) alike?

Both solutions...