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Homework Statement
A 0.085 M aqueous solution of a weak base is known to be 1.6 percent ionized. Calculate the pH of the solution.
Homework Equations
%Ionization= ([OH-] derived from base/ initial [base]) x 100%
pOH=-log[OH-}
The Attempt at a Solution
%Ionization= ([OH-] derived from base/ initial [base]) x 100%
1.6%=[OH]/0.085M
[OH]=0.136M
pOH=-log[OH-]
pOH=-log(o.136M)
pOH=0.866
pH+pOH=14, 14-0.866=13.134...
I normally do these without a problem, so I'm assuming it's a stupid mistake. The problem clearly says weak base...Where am I going wrong?
Regards,
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