![[H^+]= 0.25\times0.03 = 0.0075 M](/tpl/images/0230/8770/78a73.png)
![[A^{-}]= 0.25 \times 0.03 = 0.0075 M](/tpl/images/0230/8770/ebbeb.png)
![Ka= \frac{[H^+][A^{-}]}{[HA]}](/tpl/images/0230/8770/b86b3.png)
![pH = -log [H^+]](/tpl/images/0230/8770/9b8d2.png)
![H^+[\tex] = 0.0075 M](/tpl/images/0230/8770/51649.png)
If a weak acid, ha, is 3% dissociated in a 0.25 m
solution, calculate the ka and the ph of the...
Chemistry, 14.09.2019 05:20 selena5713
If a weak acid, ha, is 3% dissociated in a 0.25 m
solution, calculate the ka and the ph of the solution.
Answers: 1
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