What is the pOH of an aqueous solution at 25.0 #"^o#C that contains #3.98 x 10^-9# M hydronium ion?

1 Answer
anor277
Nov 6, 2016

#pOH=-log_(10)[""^(-)OH]=5.60#

Explanation:

We know or should know that under standard conditions (the which operate here): #pH+pOH=14#.

#pH=-log_(10)[H_3O^+]# #=# #-log_(10)[3.98xx10^-9]=8.40#.

And thus #pOH=14-8.60=5.60#

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