Module 6: Acids and Bases Revision

According to the Bronsted-Lowry theory, bases are:

• Always oxides and hydroxides of metals

• Alkalis which are soluble in water

• proton donors

• proton acceptors

An acidic solution is found to have a pH of 2. This solution could be:

• 0.2 mol/L HCl

• 0.01 mol/L HCl

• 0.2 mol/L H₂SO₄

• 0.01 mol/L H₂SO₄

The pH of a solution of 0.001 mol/L NaOH is:

• 3

• 11

• 1 x 10^-3

• 1 x 10^-11

The end point of a titration is the

• end of the reaction.

• point where the indicator changes colour

• equivalence point of the reaction

• Point where equal moles of reactant are present.

A solution of 0.001 mol/L solution of sulphuric acid could be classified as a

• Weak Solution of a weak acid

• Dilute solution of a strong acid

• dilute solution of a concentrated acid

• Concentrated solution of a strong acid

A solution of hydrochloric acid is diluted. As a result, its pH changes from 2 to 4. The hydrogen ion concentration of the diluted solution is:

• doubled

• halved

• increased 100 times

• decreased 100 times

Which of the following substances is an acid according to both the Arrhenius theory and the Bronsted-Lowry theory?

• NaOH

• SO₂

• NaHSO₄

• HCl

In which of these equations is water acting as a Bronsted-Lowry acid?

• NH₃ + H₂O ↔ NH₄⁺ + OH^-

• H₂PO₄^- + H₂O ↔ HPO₄^2- + H₃O⁺

• HCl + H₂O ↔ Cl^- + H₃O⁺

• NiCl₂.6H₂O ↔ NiCl₂ + 6H₂O

Which compound would form a basic aqueous solution?

• sodium ethanoate

• ammonium ethanoate

• ammonium chloride

• carbon dioxide

Which substance is basic?

• sugar solution

• baking soda

• orange juice

• lemonade