Table 4.2 summarizes the names, formulas, and classifications of some common acids and bases.
When an acid and a base are mixed in stoichiometric proportions, their acidic and basic properties disappear as the result of a neutralization reaction.
Because the salts that form in neutralization reaction are generally strong electrolytes, we can write the neutralization reaction as an ionic equation.
When the spectator ions are removed, the net ionic equation is revealed.
This net ionic equation is the same for the neutralization reaction of any strong acid and strong base.
For the reaction of a weak acid with a strong base, a similar neutralization occurs. Consider the neutralization of HF with KOH.
|HF(aq) + KOH(aq) KF(aq) + H2O(l)
|HF(aq) + (aq) + OH-(aq)
+ F-(aq) + H2O(l)
|HF(aq) + OH-(aq) F-(aq) + H2O(l)
||net ionic equation
The weak acid HF is written as a molecular formula because its dissociation is incomplete.