# Is a solution with a pH of 10 more basic than a solution with pH 8? Why so?

In aqueous solution, $p H = - {\log}_{10} \left[{H}_{3} {O}^{+}\right]$ by definition, and so............
And thus if $p H = 10$, by definition, $\left[{H}_{3} {O}^{+}\right] = {10}^{- 10} \cdot m o l \cdot {L}^{-} 1$ with respect to ${H}_{3} {O}^{+}$.
And if $p H = 8$, by definition, $\left[{H}_{3} {O}^{+}\right] = {10}^{- 8} \cdot m o l \cdot {L}^{-} 1$ with respect to ${H}_{3} {O}^{+}$.
And thus a solution that is $\left[{H}_{3} {O}^{+}\right] = {10}^{- 10} \cdot m o l \cdot {L}^{-} 1$ with respect to ${H}_{3} {O}^{+}$ is a hundredfold LESS concentrated than when $\left[{H}_{3} {O}^{+}\right] = {10}^{- 8} \cdot m o l \cdot {L}^{-} 1$. Capisce?