Mg(s)+2HCl(aq)  →  MgCl2(aq)+H2(g) In an experiment, a student places a small piece of pure Mg(s) into a beaker containing 250.mL of 6.44MHCl(aq) . A reaction occurs, as represented by the equation above.

(a) Write the balanced net ionic equation for the reaction between Mg(s) and HCl(aq) .

Explanation:

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In this case, since the writing of a net ionic equation first implies writing the complete molecular equation:

We can see that HCl and MgCl2 are ionized because they are aqueous, thus we write:

In such a way, we can cancel out the chloride ions as they are the spectator ones to obtain the net ionic one:

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