What is pOH for a solution that is 0.565*mol*L^-1 in HClO_4(aq)?

1 Answer
anor277
Apr 26, 2017

pH+pOH=14

Explanation:

pH+pOH=14 in aqueous solution under standard conditions.

HClO_4(aq) +H_2O(l) rarr H_3O^+ + ClO_4^(-)

Now "perchloric acid" is thus stoichiometric in H_3O^+, "hydronium ion", and since pH=-log_10[H_3O^+], pH=-log_10(0.272)=0.565, and...................

pOH=14-0.565=13.4

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