Interpret acid-base titration curves to determine the intercept with pH axis, equivalence point, buffer region and points where pKa = pH or pKb = pOH.

A 25.0 mL sample of 0.20 M ethanoic acid (CH₃COOH), a weak monoprotic acid with pKₐ = 4.76, was titrated with 0.20 M sodium hydroxide (NaOH). The titration curve is shown below. Determine whether the following features of the titration curve would change if 25.0 mL of 0.20 M hydrochloric acid (HCl) was titrated with 0.20 M sodium hydroxide (NaOH) instead. Explain your reasoning. (a) The pH at the equivalence point: (1 mark) (b) The volume of NaOH required to reach the equivalence point: (1 mark)

A \ (25.0 \, \text{mL}\ ) sample of \ (0.100 \, \text{mol L}^{-1}\ ) propanoic acid \ (\text{CH}_3\text{CH}_2\text{COOH}\ , \ K_a = 1.3 \times 10^{-5}\ ) is titrated with \ (0.100 \, \text{mol L}^{-1}\ ) sodium hydroxide solution. The titration curve shows \ (\text{pH}\ ) on the \ (y\ )-axis and volume of \ (\text{NaOH}\ ) added on the \ (x\ )-axis. At which volume of added \ (\text{NaOH}\ ) does \ (\text{p}K_a = \text{pH}\ )?

A 25.0 \text{ mL} sample of 0.10 \text{ mol L}^{-1} ethanoic acid ( \text{CH}_3\text{COOH} ) is titrated with 0.10 \text{ mol L}^{-1} sodium hydroxide ( \text{NaOH} ). The p K_a of ethanoic acid is 4.76 . Determine the volume of \text{NaOH} added at the point on the titration curve where p K_a = \text{pH} .