Vinegar is a dilute water solution of acetic acid with small amounts of other
components. Calculate the pH of bottled vinegar that is 0.667 M HC_{2}H_{3}O_{2},
assuming that none of the other components affect the acidity of the solution.

HC_{2}H_{3}O_{2(aq)}
H^{+}_{(aq)} + C_{2}H_{3}O_{2}^{-}_{(aq)}

We get the value for the acid dissociation constant for this reaction from
the table above.

**x in the denominator, is considered too
small compared to 0.667, so it is ignored.

x^{2} = 1.2 x 10^{-5} x = 3.5 x 10^{-3}

[H^{+}] = 3.5 x 10^{-3} M H^{+}
pH = -log(3.5 x 10^{-3}) = 2.46