Question

Complete the reaction: $\mathrm{PbO}+2\mathrm{NaOH}\to$?

Answer 1

Completing the given reaction:

• The given equation should follow the law of conservation of mass.
• Hence, the complete balanced chemical equation can be written as:

$\underset{\left(\mathrm{Lead}\mathrm{oxide}\right)}{\mathrm{PbO}\left(\mathrm{s}\right)}+\underset{\left(\mathrm{Sodium}\mathrm{hydroxide}\right)}{2\mathrm{NaOH}\left(\mathrm{aq}\right)}\to \underset{\left(\mathrm{Sodium}\mathrm{lead}\mathrm{oxide}\right)}{{\mathrm{Na}}_2{\mathrm{PbO}}_2\left(\mathrm{s}\right)}+\underset{\left(\mathrm{Water}\right)}{{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}$

• The given reaction can be classified as an acid-base reaction, which $\mathrm{PbO}$ acts as an acid, and $\mathrm{NaOH}$ acts as a base.
• Here Lead(II) oxide reacts with Sodium hydroxide to produce Lead(II)-sodium oxide and water, which takes place at a temperature near to about $400°\mathrm{C}.$

hence, the Complete reaction is given as:$\underset{\left(\mathrm{Lead}\mathrm{oxide}\right)}{\mathrm{PbO}\left(\mathrm{s}\right)}+\underset{\left(\mathrm{Sodium}\mathrm{hydroxide}\right)}{2\mathrm{NaOH}\left(\mathrm{aq}\right)}\to \underset{\left(\mathrm{Sodium}\mathrm{lead}\mathrm{oxide}\right)}{{\mathrm{Na}}_2{\mathrm{PbO}}_2\left(\mathrm{s}\right)}+\underset{\left(\mathrm{Water}\right)}{{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}$.