Chemistry, 07.03.2020 00:05 jessicaortiz6
Using the average initial pH of your acetic acid solutions (2.96), and the average molarity of those solutions(.0602), calculate a value of Ka for acetic acid. Report your result to 3 significant figures.
Answers: 3
.
![pH=-\log [H^+]](/tpl/images/0536/6580/37e81.png)
![2.96=-\log [H^+]](/tpl/images/0536/6580/04be1.png)
![[H^+]=1.096\times 10^{-3}M](/tpl/images/0536/6580/640ad.png)
![[H^+]=[CH_3COO^-]=1.096\times 10^{-3}M](/tpl/images/0536/6580/4b8c0.png)
![[CH_3COOH]=0.0602-(1.096\times 10^{-3})=0.0591M](/tpl/images/0536/6580/19210.png)
![K_a=\frac{[CH_3COO^-][H^+]}{[CH_3COOH]}](/tpl/images/0536/6580/9c35d.png)
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Using the average initial pH of your acetic acid solutions (2.96), and the average molarity of those...
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