Answers: 3
    
     
= ?![pH=-log[H^+]](/tpl/images/0346/5539/15713.png)
![1.86=-log[H^+]](/tpl/images/0346/5539/7260c.png)
![[H^+]=0.01](/tpl/images/0346/5539/6c620.png)
![[H^+]=c\times \alpha](/tpl/images/0346/5539/4fc41.png)
![[H^+]=[ClCH_2COO^-]=0.01](/tpl/images/0346/5539/98324.png)
![K_a=1.67\times 10^{-3]](/tpl/images/0346/5539/1973d.png)
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A0.15 m solution of chloroacetic acid has a ph of 1.86. what is the value of ka for this acid?...
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