What is the pH of a .500 M solution of #HNO_3#?

1 Answer
anor277
Jun 20, 2016

#pH=0.30#

Explanation:

#HNO_3(aq) + H_2O(l) rightleftharpoonsH_3O^+ + NO_3^-#

#pH=-log_10[H_3O^+]#. Since the equilibrium lies almost entirely to the right, we take #[H_3O^+]=0.500*mol*L^-1#.

#log_10(0.500)# #=# #-0.301#, and #pH=??#

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