What's the pH of a solution of $1.5M HNO_3$ ?

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Answer 1 · 2018-02-11T22:07:04

$pH=-0.18$

By definition, $pH=-log_10[H_3O^+]$ ..

and here... $HNO_3(aq) + H_2O(l) rarr H_3O^+ +NO_3^(-)$

....the equilibrium LIES strongly to the right....and we presume that the solution is stoichiometric in $H_3O^+$ , i.e. $1.50*mol*L^-1$

And so $pH=-log_10(1.50)=-(0.176)=-0.18$

What's the pH of a solution of 1.5M HNO_31.5M HNO_3?