# Balance the following equations and write corresponding ionic and net ionic equations : ...

## Question:

Balance the following equations and write corresponding ionic and net ionic equations :

(a){eq}HBr(aq) + NH_3(aq)\rightarrow{/eq}

(b){eq}Ba(OH)_2(aq) + H_3PO_4(aq)\rightarrow{/eq}

(c){eq}HCIO_4(aq) + Mg(OH)_2(s)\rightarrow{/eq}

## Balanced Reaction Equation:

A balanced reaction equation describes the stoichiometry between the different elements and compounds involved in the reactants and products of a chemical reaction. The reaction could represent acid-base, precipitation, redox and many other possible reactions. Regardless of the reaction both sides of the equation must be balanced in both mass and charge.

All of these reactions involve an acid and a base so the resulting equations will be based on proton transfer. Full ionic equations including spectator ions, while these ions are omitted in net ionic equations. If an insoluble compound is present (low Ksp) then it remains as a solid compound regardless of the form of the equation.

Question a)

{eq}Conventional: HBr (aq) + NH_3 (aq) \rightarrow NH_4Br (aq) \\ Ionic: H^+ (aq) + Br^- (aq) + NH_3 (aq) \rightarrow NH_4^+ (aq) + Br^- (aq)\\ Net-Ionic: H^+ (aq) + NH_3 \rightarrow NH_4^+ (aq) {/eq}

Question b)

{eq}Conventional: 3Ba(OH)_2 (aq) + 2H_3PO_4 (aq) \rightarrow 6H_2O (l) + Ba_3(PO_4)_2 (s) \\ Ionic: 3Ba^{2+} (aq) + 6OH^- (aq) + 6H^+ (aq) + 2PO_4^{3-} (aq) \rightarrow 6H_2O (l) + Ba_3(PO_4)_2 (s) \\ Net-Ionic: 3Ba^{2+} (aq) + 6OH^- (aq) + 6H^+ (aq) + 2PO_4^{3-} (aq) \rightarrow 6H_2O (l) + Ba_3(PO_4)_2 (s) {/eq}

Question c)

{eq}Conventional: 2HClO_4 (aq) + Mg(OH)_2 (s) \rightarrow 2H_2O (l) + Mg(ClO_4)_2 (aq) \\ Ionic: 2H^+ (aq) + 2ClO_4^- (aq) + Mg(OH)_2 (s) \rightarrow 2H_2O (l) + Mg^{2+} (aq) + 2ClO_4^- (aq) \\ Net-Ionic: 2H^+ (aq) + Mg(OH)_2 (s) \rightarrow 2H_2O (l) + Mg^{2+} (aq) {/eq}