Exercise Solutions Neutralization

Exercises

Exercise 1. Write a balanced ionic and net ionic equation when aqueous perchloric acid is neutralized by aqueous potassium hydroxide.

Perchloric acid, HClO₄ is a strong acid and will completely dissociate. The molecular equation is:

HClO₄ (aq) + KOH (aq) → KClO₄^– (aq) + H₂O (l)

The ionic equation is:

H₃O⁺ (aq) + ClO₄^– (aq) + K⁺ (aq) + OH^– (aq) → K⁺ (aq) + ClO₄^– (aq) + 2 H₂O (l)

The net ionic equation is:

H₃O⁺ + OH^– (aq) → 2 H₂O (l)

The net ionic equation can also be written as:

H⁺ (aq) + OH^– (aq) → H₂O (l)

Exercise 2. Write a balanced net ionic equation for the neutralization of lithium hydroxide and hydrogen iodic acid.

LiOH is a strong base and HI is a strong acid. The net ionic equation is:

H₃O⁺ + OH^– (aq) → 2 H₂O (l)

The net ionic equation can also be written as:

H⁺ (aq) + OH^– (aq) → H₂O (l)

Exercise 3. Write a balanced net ionic equation for the neutralization of HClO (perchlorous acid) and LiOH.

HClO is a weak acid and does not completely dissociate. The molecular equation is:

HClO (aq) + LiOH (aq) → LiClO (aq) + H₂O (l)

Next, write the ionic equation. Recall, HClO is a weak acid and only partially dissociates.

HClO (aq) + Li⁺ (aq) + OH^– → Li⁺ (aq) + ClO^– (aq) + H₂O (l)

The net ionic equation is:

HClO (aq) + OH^– → ClO^– (aq) + H₂O (l)

Exercise 4. Write a balanced net ionic equation for sulfuric acid (H₂SO₄) being neutralized by Ba(OH)₂

Here we have a strong acid and a strong base. The net ionic equation is:

H₃O⁺ + OH^– (aq) → 2 H₂O (l)

Exercise 5. Oxalic acid (H₂C₂O₄) is a diprotic acid. Write the 2 acid dissociation equations for aqueous oxalic acid.

H₂C₂O₄ is a weak diprotic acid.

1^st dissociation: H₂C₂O₄ (aq) + H₂O (l) ⇄ HC₂O₄^– (aq) + H₃O⁺ (aq)

2^nd dissociation: HC₂O₄^– (aq) + H₂O (l) ⇄ C₂O₄^2- (aq) + H₃O⁺ (aq)