Ammonia (NH3) acts as a weak base in aqueous solution. What is the acid that reacts with this base when ammonia is dissolved in water?

What is the conjugate base of the HSO4 – (aq) ion?

If the pH of a solution increases by 2 units (e.g., from 1 to 3), then the ratio of the new to the original hydronium ion concentration is __________

What is the pH of a 0.010 M solution of acetic acid? Ka for acetic acid is 1.8 × 10–5

The pH of a popular soft drink is 3.4; what is its hydronium ion concentration?

When [H+ ] = 4.0 × 10–9 M in water at 25°C, then pH = __________

10 cm3 of 0.01 mol dm–3 nitric acid (HNO3 ) is diluted with 90 cm3 of water. What is the pH of the resulting solution?

Suggest one method, other than measuring pH, which could be used to distinguish between solutions of a strong acid and a weak acid of the same concentration. State the expected results.

In the Brønsted–Lowry definition of acids and bases, an acid __________

A solution with an [OH– ] concentration of 1.20 × 10–7 M has a pOH and pH of __________

The indicator bromophenol blue, HIn(aq), has a form that is yellow and an In– (aq) form that is blue. Write an equation to show how bromophenol blue acts as an indicator.

In the following reaction in aqueous solution CH3COOH + NH3 = CH3COO- + NH4+, the acid reactant is __________ and its conjugate base product is __________.

The first disinfectant used by Joseph Lister was called carbolic acid. This substance now is known as phenol, C6H5OH (pKa = 10.0). What is the pH of a 0.10 M solution of phenol?