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» <html><body><p></p>Solution :Concentrationof `HNO_(3)` solution = 0.<a href="https://interviewquestions.tuteehub.com/tag/63-330460" style="font-weight:bold;" target="_blank" title="Click to know more about 63">63</a> g <a href="https://interviewquestions.tuteehub.com/tag/per-590802" style="font-weight:bold;" target="_blank" title="Click to know more about PER">PER</a> <a href="https://interviewquestions.tuteehub.com/tag/100-263808" style="font-weight:bold;" target="_blank" title="Click to know more about 100">100</a> <a href="https://interviewquestions.tuteehub.com/tag/ml-548251" style="font-weight:bold;" target="_blank" title="Click to know more about ML">ML</a> (Given) <br/> `=6.3 g ` per litre `= (6.3)/(63) ` moles/litre = `10^(-1)M` (`:' ` Mol. Mass of `HNO_(3) = 63`) <br/> Now, `HNO_(3)`, completely ionizes as : `HNO_(3)H_(2)O rarrH_(3)O^(+)+NO_(3)^(-)` <br/> `:. [H_(3)O^(+)]=[HNO_(3)]=10^(-1)M :. pH = - log [H_(3)O^(+)]= - log 10^(-1)=1`</body></html>