3.14 - The ionic equation for neutralisation

3.14 - The ionic equation for neutralisation

In acid–alkali neutralisation, hydrogen ions and hydroxide ions react to form water. You will write the ionic equation, check its atoms and charge, and distinguish the reacting ions from ions that remain unchanged in solution.

The reacting ions

An aqueous acid supplies hydrogen ions, H+(aq)H^+(aq). An alkali supplies hydroxide ions, OH−(aq)OH^-(aq). The symbol (aq)(aq) means dissolved in water.

These ions react to form water:

Ionic equation for neutralisation

H+(aq)+OH−(aq)→H2O(l)H^+(aq) + OH^-(aq) \rightarrow H_2O(l)

There are two hydrogen atoms and one oxygen atom on each side. The total charge on the left is +1+(−1)=0+1 + (-1) = 0, matching neutral water on the right. The product is water, H2OH_2O, rather than hydrogen gas, H2H_2.

Hydrogen and hydroxide ions form water

The circles labelled with ion formulae are symbols for the reacting ions. The water model shows one oxygen atom joined to two hydrogen atoms.

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