${\mathbf{K}}_{\mathbf{a}}\mathbf{}\mathbf{=}\frac{\left[{\mathrm{CH}}_{3}{\mathrm{COO}}^{-}\right]\left[{H}_{3}{O}^{+}\right]}{\left[{\mathrm{CH}}_{3}\mathrm{COOH}\right]}\phantom{\rule{0ex}{0ex}}{\mathbf{K}}_{\mathbf{a}}\mathbf{}\mathbf{=}\frac{\left(x\right)\left(x\right)}{\mathbf{0}\mathbf{.}\mathbf{150}\mathbf{}\mathbf{-}\mathbf{}\mathbf{x}}$

$\frac{{\left[{\mathrm{CH}}_{3}\mathrm{COOH}\right]}_{\mathbf{initial}}}{{\mathbf{K}}_{\mathbf{a}}}\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{0}\mathbf{.}\mathbf{150}}{\mathbf{1}\mathbf{.}\mathbf{8}\mathbf{\times}{\mathbf{10}}^{\mathbf{-}\mathbf{5}}}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{}\mathbf{500}$

A 35.0-mL sample of 0.150 M acetic acid (CH_{3}COOH) is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added.

0 mL of the base

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