Question

Write balanced equations (all three types) for the reactions that occur when the following aqueous solutions are mixed.

a. ammonia (aqueous) and nitric acid

b. barium hydroxide (aqueous) and hydrochloric acid

c. perchloric acid [${\mathrm{HClO}}_4\left(\mathrm{aq}\right)$ ] and solid iron(III)hydroxide

d. solid silver hydroxide and hydrobromic acid

Short answer

The balanced equations for the reactions:

1. ${\mathrm{NH}}_3\left(\mathrm{aq}\right)+{\mathrm{HNO}}_3\left(\mathrm{aq}\right)\to {\mathrm{NH}}_4{\mathrm{NO}}_3\left(\mathrm{aq}\right)$
2. $\mathrm{Ba}{\left(\mathrm{OH}\right)}_2\left(\mathrm{aq}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)\to {\mathrm{BaCl}}_2\left(\mathrm{aq}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$
3. $3{\mathrm{HClO}}_4\left(\mathrm{aq}\right)+\mathrm{Fe}{\left(\mathrm{OH}\right)}_3\left(\mathrm{s}\right)\to \mathrm{Fe}{\left({\mathrm{ClO}}_4\right)}_3\left(\mathrm{aq}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$
4. $\mathrm{AgOH}\left(\mathrm{s}\right)+\mathrm{HCl}\left(\mathrm{aq}\right)\to \mathrm{AgCl}\left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

Step-by-step solution

Definition 

A balanced chemical equation is one in which the number of atoms present in thereactant side of the equation equals the number of atoms present in the product side of the equation.

Determination of balanced equations for the reaction between ammonia (aqueous) and nitric acid

a)

The balanced molecular equation:

${\mathrm{NH}}_3\left(\mathrm{aq}\right)+{\mathrm{HNO}}_3\left(\mathrm{aq}\right)\to {\mathrm{NH}}_4{\mathrm{NO}}_3\left(\mathrm{aq}\right)$

Ammonium nitrate is formed when ammonia and nitric acid react. This is an example of an acid-base reaction.

The whole ionic equation is as follows:

${\mathrm{NH}}_3\left(\mathrm{aq}\right)+{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{NO}}_3^{-}\left(\mathrm{aq}\right)\to {\mathrm{NH}}_4^{+}+{\mathrm{NO}}_3^{-}\left(\mathrm{aq}\right)$

Cancel the spectator ions on both sides, i.e. ${\mathrm{NO}}_3^{-}$,

Net ionic equation:

${\mathrm{NH}}_3\left(\mathrm{aq}\right)+{\mathrm{H}}^{+}\left(\mathrm{aq}\right)\to {{\mathrm{NH}}_4}^{+}\left(\mathrm{aq}\right)$

Determination of balanced equations for the reaction between barium hydroxide (aqueous) and hydrochloric acid

b)

The balanced molecular equation:

$\mathrm{Ba}{\left(\mathrm{OH}\right)}_2\left(\mathrm{aq}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)\to {\mathrm{BaCl}}_2\left(\mathrm{aq}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

When barium hydroxide reacts with hydrochloric acid, barium chloride and water is formed. This is an acid-base reaction with a two-fold displacement.

The total ionic equation:

${\mathrm{Ba}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)+2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)\to {\mathrm{Ba}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

Cross out spectator ions on both sides, i.e. ${\mathrm{Ba}}^{2+},{\mathrm{Cl}}^{-}$,

Net ionic equation:

$2{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)+2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)\to 2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

Determination of balanced equations for the reaction between perchloric acid [ HClO4(aq)] and solid iron (III) hydroxide

c)

The balanced molecular equation:

$3{\mathrm{HClO}}_4\left(\mathrm{aq}\right)+\mathrm{Fe}{\left(\mathrm{OH}\right)}_3\left(\mathrm{s}\right)\to \mathrm{Fe}{\left({\mathrm{ClO}}_4\right)}_3\left(\mathrm{aq}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

Iron (III) per chlorate and water are formed when perchloric acid reacts with iron (III) hydroxide. This is an acid-base double displacement reaction.

The total ionic equation:

$3{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+3{\mathrm{ClO}}_4^{-}\left(\mathrm{aq}\right)+\mathrm{Fe}{\left(\mathrm{OH}\right)}_3\left(\mathrm{s}\right)\to {\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+3{\mathrm{ClO}}_4^{-}\left(\mathrm{aq}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

Cross out spectator ions on both sides, i.e.${\mathrm{ClO}}_4^{-}$,

Net ionic equation:

$3{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+\mathrm{Fe}{\left(\mathrm{OH}\right)}_3\left(\mathrm{s}\right)\to {\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

Determination of balanced equations for the reaction between solid silver hydroxide and hydrochloric acid

d)

The balanced molecular equation:

$\mathrm{AgOH}\left(\mathrm{s}\right)+\mathrm{HCl}\left(\mathrm{aq}\right)\to \mathrm{AgCl}\left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

Silver chloride and water are formed when silver hydroxide reacts with hydrochloric acid. This is an acid-base double displacement reaction.

The total ionic equation:

$\mathrm{AgOH}\left(\mathrm{s}\right)+{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)\to \mathrm{AgCl}\left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

There are no spectator ions.

Net ionic equation:

$\mathrm{AgOH}\left(\mathrm{s}\right)+{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)\to \mathrm{AgCl}\left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$