Question #44092

A buffer solution is to be prepared using acetic acid (\ce{CH3COOH}) and sodium acetate (\ce{CH3COONa}) in a $60\%$ (v/v) ethanol-water mixed solvent at $298\text{ K}$. The aqueous $pK_a$ of acetic acid is $4.76$. The standard free energy of transfer ($\Delta G^\circ_{tr}$) for the dissociation reaction $\ce{CH3COOH \rightleftharpoons CH3COO- + H+}$ from pure water to the mixed solvent is $+5.70\text{ kJ mol}^{-1}$ due to the lower dielectric constant of the medium. (Given: $2.303 RT = 5.70\text{ kJ mol}^{-1}$ at $298\text{ K}$).

Which of the following correctly identifies (i) the pH at which this buffer exhibits maximum buffer capacity in the mixed solvent, and (ii) the required molar ratio of $\frac{[\ce{CH3COONa}]}{[\ce{CH3COOH}]}$ to prepare a buffer of $\text{pH} = 4.76$ in this specific medium?