Upon introduction of additional solutes to water, we observe a boiling point elevation according to the colligative properties. This means that when CH3COOH
are introduced to solution, boiling point increases, and vapor pressure decreases accordingly. An ion-dipole interaction occurs when ions interact with molecules bearing partial charges. Because CH3COOH
is a weak acid, it is undoubtedly polar. In the protonated form, the partial negative oxygen and the partial positive carbon will display ion-dipole interactions with Na+
, respectively. In the deprotonated form, ionic bonding will be observed between CH3COO− and Na+
. Lastly, any solution of pure water with acidic solute will be more acidic than pure water, regardless of the concentration of acid. Although a tiny concentration of acid may have a minuscule effect on water pH, a change exists.