# Write the net ionic equation for the following reaction: {eq}Zn(s) + H_2SO_4(aq) \to ZnSO_4(aq) + H_2(g) {/eq}

## Question:

Write the net ionic equation for the following reaction: {eq}Zn(s) + H_2SO_4(aq) \to ZnSO_4(aq) + H_2(g) {/eq}

## Net Ionic Equation:

An ionic equation is a type of chemical equation applicable to reaction systems occurring in aqueous solution. Therefore, the molecular version of the chemical equation contains some number of species present with aqueous "aq" phase notation. Examples include acid-base (proton transfer), redox (electron transfer) and precipitation reaction systems. The ionic equation is differentiated from the molecular version by writing all dissociated species in terms of their ionic components. The net ionic equation is derived from the ionic equation by eliminating spectator ion species. These are ions that are not actively participating in the reaction of interest.

The given molecular reaction equation is:

{eq}\rm Zn(s) + H_2SO_4(aq) \to ZnSO_4(aq) + H_2(g) {/eq}

This equation represents a redox reaction occurring between zinc metal and sulfuric acid. It is also an example of a single displacement reaction between the zinc and hydrogen atoms. The zinc will be oxidized from the zero state in the metal to the +2 state in zinc (II) sulfate. Simultaneously, the hydrogen atoms are reduced from the +1 state in sulfuric acid to zero in hydrogen gas. Sulfuric acid is a strong diprotic acid and zinc sulfate is a soluble salt compound species. The ionic equation is:

{eq}\rm Zn (s) + 2H^+ (aq) + SO_4^{2-} (aq) \rightarrow Zn^{2+} (aq) + SO_4^{2-} (aq) + H_2 (g) {/eq}

We see that the compound sulfate anion is repeated on both sides. This indicates that it is a spectator ion, so we remove it in the net ionic equation:

{eq}\rm Zn (s) + 2H^+ (aq) \rightarrow Zn^{2+} (aq) + H_2 (g) {/eq}