Question

Write the overall, ionic and net ionic equations for the following reaction. Perchloric acid (HClO4) and barium hydroxide (Ba(OH)2)

Answer 1

The reaction of perchloric acid and barium hydroxide yields to barium perchlorate (Ba(ClO4)2) and water (H2O). The resulting balanced equation is 2 HClO4 + Ba(OH)2 = Ba(ClO4)2 +2 H2O. This means, for every mole of barium perchlorate produced, 2 moles of perchloric acid and barium hydroxide are required.

Answer 2

Answer : The net ionic equation will be,

$2H^+(aq)+2OH^-(aq)\rightarrow 2H_2O(l)$

Explanation :

In the net ionic equations, we are not include the spectator ions in the equations.

Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.

The given balanced ionic equation will be,

$2HClO_4(aq)+Ba(OH)_2(aq)\rightarrow Ba(ClO_4)_2(aq)+2H_2O(l)$

The ionic equation in separated aqueous solution will be,

$2H^+(aq)+2ClO_4^-(aq)+Ba^{2+}(aq)+2OH^-(aq)\rightarrow 2H_2O(l)+Ba^{2+}(aq)+2ClO_4^-(aq)$

In this equation, $ClO_4^-\text{ and }Ba^{2+}$ are the spectator ions.

By removing the spectator ions from the balanced ionic equation, we get the net ionic equation.

The net ionic equation will be,

$2H^+(aq)+2OH^-(aq)\rightarrow 2H_2O(l)$