[StaticRoar]

Problem: The pH of a solution of 0.16M GaCl3 is measured to be 3.96.
 
Ga(H2O)6^(3+)(aq) <--> Ga(OH)(H2O)5^(2+)(aq) + H+(aq)
 
What is the equilibrium constant for the reaction?
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Attempt at Solution:
 
[H+]=10^(-3.96)=1.1x10^(-4) M
 
Using an ICE table, k=(1.1x10^(-4))^(2)/(0.16-x), where x=1.1x10^(-4)
 
Plug in the value of x, and find k.
 
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Not too familiar with these types of problems so I'm not sure I have it right. Is the process correct?

[Borek]

Looks OK to me.

[StaticRoar]

Thanks.