# For the reaction Mg(NO_3)_2(aq) + H_2SO_4(aq) \to ?, write: (1) a balanced chemical equation...

## Question:

For the reaction {eq}\displaystyle Mg(NO_3)_2(aq) + H_2SO_4(aq) \to \ ? {/eq}, write:

(1) a balanced chemical equation (molecular equation),

(2) a total ionic equation, and

(3) a net ionic equation. Include the appropriate phase for each species.

## Net Ionic Equations:

Many different types of chemical equations can be written to represent a reaction. The chemical equation that shows the compounds and molecules involved is the molecular equation. For reactions that occur in aqueous solutions, a net ionic equation can be used. The net ionic equation shows the substances directly involved in the formation of product.

The products of the reaction are magnesium sulfate and nitric acid. By exchanging the ions of the reactants with one another, the balanced molecular equation is obtained.

{eq}\rm Mg(NO_3)_2(aq) + H_2SO_4(aq) \to MgSO_4(aq) + 2HNO_3(aq) {/eq}

By separating the strong electrolytes into ions, the following total ionic equation is obtained. The first dissociation of sulfuric acid proceeds completely. The second ionization does not proceed completely. For this reason, the bisulfate ion is formed.

{eq}\rm Mg^{2+}(aq) + 2NO_3^-(aq) + H^+(aq) + HSO_4^-(aq) \to Mg^{2+}(aq) + SO_4^{2-}(aq) + 2H^+(aq) + NO_3^-(aq) {/eq}

The net ionic equation is obtained by removing the ions that appear on both sides of the chemical equation.

{eq}\rm HSO_4^-(aq) \to SO_4^{2-}(aq) + H^+(aq) {/eq}