Answers: 2
![pH=-log([H^+]})](/tpl/images/0726/6480/27fdb.png)
![[H^+]=10^{-pH}=10^{-4.0}=1x10^{-4}M](/tpl/images/0726/6480/17ea8.png)
) is computed as:
is 0.010 M and the acid dissociation constant is:
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A 0.010 M aqueous solution of a weak acid HA has a pH of 4.0. What is the degree of ionization of HA...
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