# Write the balanced complete ionic equation for the following reaction: K3PO4(aq) + NiCl2(aq)...

## Question:

Write the balanced complete ionic equation for the following reaction:

{eq}K_3PO_4(aq) + NiCl_2(aq) \to Ni_3(PO_4)_2(s) + KCl(aq) {/eq}

## Complete Ionic Equation

The complete ionic equation is an ionic equation that shows all of the particles in a solution as they realistically exist.

The compounds in Aqueous state ({eq}\rm aq {/eq} as the symbol) will separate into their constituent ions. If we write the equation with its constituent ions, then we call the equation a complete ionic equation. For example,

{eq}\rm HCl (aq) + NaOH (aq) \to NaCl (aq) + H_2O (l) {/eq}

{eq}\rm HCl {/eq}, {eq}\rm NaOH {/eq}, and {eq}\rm NaCl {/eq} will be dissociated into their ions, but {eq}\rm H_2O {/eq} will be undissociated.

{eq}\rm H^+ (aq) + Cl^- (aq) + Na^+ (aq) + OH^- (aq) \to Na^+ (aq) + Cl^- (aq) + H_2O (l) {/eq}

That is a complete ionic equation.

First, we will write a balanced molecular chemical equation.

{eq}\rm 2K_3PO_4 (aq) + 3NiCl_2 (aq) \to Ni_3(PO_4)_ 2(s) + 6KCl (aq) {/eq}

Second, we will write the balanced complete ionic equation for the reaction.

We will separate the Aqueous (aq) compounds into their constituent ions.

{eq}\rm 6 K^+ (aq) + 2 PO_4^{3-} (aq) + 3Ni^{2+} (aq) + 6 Cl^- (aq) \to Ni_3(PO_4)_ 2(s) + 6 K^+ (aq) + 6 Cl^- (aq) {/eq}

Therefore, the balanced complete ionic equation for the following reaction:

{eq}\rm 6 K^+ (aq) + 2 PO_4^{3-} (aq) + 3Ni^{2+} (aq) + 6 Cl^- (aq) \to Ni_3(PO_4)_ 2(s) + 6 K^+ (aq) + 6 Cl^- (aq) {/eq}