The dissociation constant of a weak monoacidic base is 10^-5. The pH o

1.	The dissociation constant of a weak monoacidic base is 10^-5. The pH of its 0.1 M solution will be approximately to to
Answer» Hey there! we know that , For a weak ACID, [H + ]= $\sqrt{kac}$ The dissociation constant is 10^ −5 and the concentration is 0.1 M. Let us now substitute the VALUES in our formula : [H +] = $\sqrt{(1 10^-5) 0.1}$ = $\sqrt{1* 10^-6}$ = 1 * $10^{-3}$ pH = −log[H + ] = $- log10 ^{-3}$ = $-(-3)log_{10}$ = $3log_{10}$ = 3 ( $log_{10} = 1$ ) #Hope it helps!