Chemistry, 23.02.2020 05:56 isaacbryan2416
A certain weak acid, HA, has a Ka value of 2.6×10−7. Calculate the percent ionization of HA in a 0.10 M solution.
Answers: 3
![PI=\frac{[A-]}{[HA]} x100](/tpl/images/0520/5455/031dd.png)
![Ka=\frac{[H+][A-]}{[HA]}\\ \\](/tpl/images/0520/5455/b886f.png)
![Ka=\frac{[H+]^{2} }{[HA]} \\\\](/tpl/images/0520/5455/c597e.png)
![[H+]=\sqrt[2]{Ka.[HA]} \\\\](/tpl/images/0520/5455/88b1b.png)
![[H+] =\sqrt{(2,610^{-7} )(0,1)} = 1,61210^{-4}](/tpl/images/0520/5455/d2b22.png)
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A certain weak acid, HA, has a Ka value of 2.6×10−7. Calculate the percent ionization of HA in a 0.1...
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