Acid Base Practice

Which of the following is a strong base?

• Potassium hydroxide

• Hydrogen chloride

• NaHCO₃

• Ammonia

Four aqueous solutions, I, II, III and IV, are listed below.

I. 0.100 mol dm-3 HCl

II. 0.010 mol dm-3 HCl

III. 0.100 mol dm-3 NH₄⁺

IV. 0.010 mol dm-3 NaOH

What is the correct order of increasing [H+] of these solutions?

• IV, 3, II, I

• I, II, IV, III

• II, I, III, IV

• II, I, IV, III

Which substance can be dissolved in water to give a 0.1 mol dm-3 solution with a low [H+] and a high electrical conductivity?

• NaOH

• HCl

• NaCl

• NH3

Which species are a conjugate pair according to the Brønsted-Lowry theory?

• H₂SO₄ and HSO₄-

• CH₃COOH and CH₃CHO

• NH₃ and BF₃

• H₂NO₃ + and NO₃-

Which is not a strong acid?

• carbonic acid

• nitric acid

• sulfuric acid

• hydrochloric acid

Which is a Brønsted-Lowry acid-base pair?

• CH₃COOH and CH₃COO-

• NH₄+ and NH₂-

• H₂SO₄ and SO₄²⁻

• H₂O and O₂⁻

Solutions of hydrochloric acid (HCl) and ethanoic acid (CH₃COOH) of the same concentration and volume reacted completely with 5.0 g of calcium carbonate in separate containers. Which statement is correct?

• The same volume of CO₂(g) was produced with both CH₃COOH and HCl.

• CH₃COOH reacted slower because it has a a higher [H+] than HCl.

• A smaller volume of CO₂(g) was produced with CH₃COOH than with HCl.

• A greater volume of CO₂(g) was produced with CH₃COOH than with HCl.

Which methods will distinguish between equimolar solutions of a strong base and a strong acid?

I. Add magnesium to each solution and look for the formation of gas bubbles.

II. Add aqueous sodium hydroxide to each solution and measure the temperature change.

III. Use each solution in a circuit with a battery and lamp and see how bright the lamp glows.

• I and II only

• I and III only

• II and III only

• I, II and III

In the below equilibrium, what is the conjugate acid of A⁻?

HA + H₂O → H₃O⁺ + A–

• HA

• H₂O

• H₃O⁺

• OH-

What does it mean for this equilibrium to have a very large K?

• A is a weak base

• A is a weak acid

• 1 is a weak base

• 1 is a weak acid