Question #8a714

1 Answer
anor277
Dec 22, 2016

#pH=12#

Explanation:

#[HO^-]=(4*g)/(39.99*g*mol^-1)xx1/(10*L)=0.01*mol*L^-1#.

Now #pOH=-log_10[HO^-]=-log_10(0.01)=2.0#

But #pH+pOH=14#, and thus #pH=12#

That #pH+pOH=14# is key, and of course it stems from the autoprotolysis equilibrium, #[HO^-][H_3O^+]=10^-14#.

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