The explanation of substituent effects on the acidity of substituted carboxylic acids usually focuses on two factors: (a) The ability of the substituent to stabilize the negative charge; and (b) the effect of solvation on the anion. However, there will also be substituent effects on the stability and solvation of the undissociated acid. The studies described on p. XXX resulted in the following values for the gas phase energy (in hartrees) of the acids and anions and the resulting $\Delta G$ for gas phase ionization. Using this information and the solvation energies on p. 53 ,analyze the relative importance of intrinsic anion stabilization and solvation or the observed acidity.
\begin{tabular}{lccc}
\hline \multicolumn{1}{c}{$\mathrm{x}$} & Acid, $E_{\text {gs }}$ & Anion, $E_{\text {gu }}$ & $\Delta G($ kcal/mol $)$ \\
\hline $\mathrm{H}$ & $-189.551612$ & $-189.005818$ & $342.49$ \\
$\mathrm{CH}_{3}$ & $-228.792813$ & $-228.241528$ & $345.94$ \\
$\mathrm{ClCH}_{2}$ & $-687.945725$ & $-687.414262$ & $333.50$ \\
$\mathrm{NCCH}_{2}$ & $-320.909115$ & $-320.386960$ & $327.66$ \\
$\left(\mathrm{CH}_{3}\right)_{3} \mathrm{C}$ & $-346.481196$ & $-345.936639$ & $341.71$ \\
\hline
\end{tabular}