Calculate the pH of a solution that contains 1.00 M HF (K_(a)=7.2xx10^(-4)) and 5.00M HClO (K_(a)=3.5xx10^(-8)).

Calculate the pH of a solution that contains 1.00 M HF (K_(a)=7.2xx10^

1.	Calculate the pH of a solution that contains 1.00 M HF (K_(a)=7.2xx10^(-4)) and 5.00M HClO (K_(a)=3.5xx10^(-8)).
Answer» Solution :As `K_(a)` for `HClO lt ltK_(a)` for HF, `[H_(3)O^(+)]` obtained from HClO can be neglected in comparison to `[H_(3)O^(+)]` obtained from HF. HENCE `[H_(3)O^(+)]=SQRT(K_(a) (HF)xxC(HF))=sqrt((7.2xx10^(-4))(1.0))=2.68xx10^(-2)M` `pH = - log (2.68 xx 10^(-2))=2-0.4265 = 1.57` (approx)