Answers: 3
![Ka_1=\frac{[H^+][HA^-]}{[H_2A]}](/tpl/images/0847/3563/40a10.png)
![[H^+]=[HA^-]=10^{-pH}=10^{-1.47}=0.0339M](/tpl/images/0847/3563/389eb.png)
![[H_2A]=\frac{19.5g/(104.06 g/mol)}{0.250L}=0.750M](/tpl/images/0847/3563/b8a4c.png)
![[H^+]=[A^-^2]=10^{-4.26}=5.50x10^{-5}M](/tpl/images/0847/3563/18ffb.png)
![Ka_2=\frac{[H^+][A^{-2}]}{[HA^-]}=\frac{(5.50x10^{-5})(5.50x10^{-5})}{0.300-(5.50x10^{-5})}\\ \\Ka_2=1.01x10^{-8}](/tpl/images/0847/3563/0e92d.png)
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The pH of a solution of 19.5 g of malonic acid in 0.250 L is 1.47.The pH of a 0.300 M Solution of so...
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