Question

8. Use the half-reaction method to balance the following equation and then identify the oxidizing and reducing agents:

Fe(OH)2 (s) + Pb(OH)3 -(aq) → Fe(OH)3 (s) + Pb(s) [basic]

Answer 1

The given reaction is as follows

Pb(OH)₃ ^- (aq) $\longrightarrow Pb(s)$

$Fe(OH)_2 \longrightarrow Fe(OH)_3$

Now balance other atom except O and H

Pb(OH)₃ ^- (aq) $\longrightarrow Pb(s)+3H_2O$

$Fe(OH)_2 + H_2O \longrightarrow Fe(OH)_3$

Now balance H and H⁺ ions and add electrons

half balance reaction s

$Pb(OH)_3^- (aq) +3H^+ +2e^- \longrightarrow Pb(s) + 3H_2O$

$2Fe(OH)_2 + 2H_2O \longrightarrow 2Fe(OH)_3 +2H^+ +2e^-$

on combining both equation we get

$Pb(OH)_3^- (aq) +2Fe(OH)_2 \longrightarrow Pb(s) + Fe(OH)_3(s) + OH^{-1} (aq)$

oxidizing agent - Pb(OH)₃^-

reducing agent Fe(OH)₂