Chemistry, 04.08.2019 05:00 pwolfiimp4
A0.15 m solution of a weak acid is 3.0 dissociated. calculate ka
Answers: 1
= 0.03
![c-c\alpha=[0.15-(0.15\times 0.03)]=0.1455M](/tpl/images/0168/2409/30903.png)
![[H^+]=c\alpha =[0.15\times 0.03]=0.0045M](/tpl/images/0168/2409/94967.png)
![[A^-]=c\alpha =[0.15\times 0.03]=0.0045M](/tpl/images/0168/2409/00b5d.png)
for above equation follows:![K_{a}=\frac{[H^+][A^-]}{[HA]}](/tpl/images/0168/2409/959fb.png)
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A0.15 m solution of a weak acid is 3.0 dissociated. calculate ka...
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