The pH of a dilute sample of ethanoic acid is measured. The equation showing the partial dissociation of ethanoic acid is given below. $\text{CH}_3\text{COOH}(aq) \rightleftharpoons \text{CH}_3\text{COO}^-(aq) + \text{H}^+(aq)$ Aqueous sodium ethanoate, $\text{CH}_3\text{COONa}$, is then added to the dilute ethanoic acid, and the pH is measured once more. What is the starting pH of the dilute ethanoic acid, and what happens to it after aqueous sodium ethanoate has been added?
Chemistry 5070 · O Level · The characteristic properties of acids and bases