Between 0.1(M) and 0.01(M) acetic acid solutions which one will have a higher pH, and why?

Explanation

In an aqueous solution of a weak monoprotic acid (e.g., `CH_(3)COOH`), `[H_(3)O^(+)]=sqrt(cxxK_(a))`, where c=molar concentration of the solution and `K_(a)=`ionisation constant of the weak acid.
Therefore, in 0.1(M) `CH_(3)COOH` solution `[H_(3)O^(+)]=sqrt(0.1xxK_(a))mol*L^(-1)` and in 0.01(M) `CH_(3)COOH` solution, `[H_(3)O^(+)]=sqrt(0.01 xxK_(a))mol*L^(-1)` Hence, the concentration of `H_(3)O^(+)` ions in 0.1(M) `CH_(3)COOH` solution will be more than that in 0.01(M) `CH_(3)COOH` solution. therefore, the pH of 0.01(M) `CH_(3)COOH` solution will be greater than that of 0.19M) `CH_(3)COOH` solution.