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#