A solution is found to contain 0.63 g of nitric acid per 100 ml of the solution . What is the pH of the solution if the acid is completely dissociated ?

A solution is found to contain 0.63 g of nitric acid per 100 ml of the

1.	A solution is found to contain 0.63 g of nitric acid per 100 ml of the solution . What is the pH of the solution if the acid is completely dissociated ?
Answer» Solution :Concentrationof `HNO_(3)` solution = 0.63 g PER 100 ML (Given) `=6.3 g ` per litre `= (6.3)/(63) ` moles/litre = `10^(-1)M` (`:' ` Mol. Mass of `HNO_(3) = 63`) Now, `HNO_(3)`, completely ionizes as : `HNO_(3)H_(2)O rarrH_(3)O^(+)+NO_(3)^(-)` `:. [H_(3)O^(+)]=[HNO_(3)]=10^(-1)M :. pH = - log [H_(3)O^(+)]= - log 10^(-1)=1`