# What happens in a buffer when the level of H+ ions in solution increases?

The protium ion reacts with the base, and $p H$ is marginally diminished.
$p H = p {K}_{a} + {\log}_{10} \left\{\frac{\left[{A}^{-}\right]}{\left[H A\right]}\right\}$ .
Should ${H}^{+}$ be added to the buffer, ${A}^{-}$ would be protonated and $\left[H A\right]$ would increase, and given the equation $p H$ would decrease marginally. On the other hand, in an unbuffered solution, $p H$ would decrease prodigiously should a strong acid be added to the solution.