Acid and Bases Revision

Which one of the following represents a concentrated

solution of a weak acid?

• 6.0 M CH₃COOH

• 0.01 M CH₃COOH

• 6.0 M HCl

• 0.01 M HCl

Which one of the following can act as either a

Brønsted–Lowry acid or base in aqueous solutions?

• HS^–

• NH₄⁺

• CO₃^2–

• CH₄

Which of the following acids can be classified as

polyprotic in water?

I - CH₃COOH

II - H₂SO₃

III - NH₄⁺

• I only

• II only

• I and II only

• I, II and III

A solution of NaOH has a pH of 13 at 25ºC. What mass,

in g, of sodium hydroxide is present in 500 mL of this

solution?

• 2.0

• 0.050

• 2.0 x 10^–12

• 4.0

Which one of the following is the conjugate base of

OH^–?

• H₂O

• O^2–

• H₃O⁺

• NaOH

Which reactions can be classified as acid–

base reactions?

• 2Mg(s) + O₂(g) → 2MgO(s)

• Ca(s) + 2H⁺(aq) → Ca²⁺(aq) + H₂(g)

• HCOOH(aq) + H₂O(l) → HCOO^–(aq) + H₃O⁺(aq)

• 2Br^–(aq) + Cl₂(aq) → Br₂(aq) + 2Cl^–(aq)

Define the terms 'strong' and 'weak' acid

HCO3^– is an amphiprotic ion. Write chemical

equations to show it acting in water as:

i a base

ii an acid.

Calculate the OH^- concentration when the concentration of HNO₃ is 0.20M

• 2.0 x 10^-13 M

• 5.0 x 10^-14 M

• 6.0 x 10^-11 M

• 0.50M

Calculate the H₃0⁺ concentration when a solution of HCl has a concentration of 0.75M

• 0.55M

• 0.60M

• 0.75M

• 6.0 x 10^-12 M