You are given 10.00 mL of a solution of an unknown acid. The pH of this solution is exactly 2.95. You determine that the concentration of the unknown acid was 0.1224 M. You also determined that the acid was monoprotic (HA). What is the K_a and pK_a of your unknown acid
Answers: 2
is dissociation constant and the value of 
is 4.98.![pH=-\log[H^+]](/tpl/images/0548/6523/cf945.png)
![2.95=-\log[H^+]](/tpl/images/0548/6523/b4bb5.png)
![[H^+]=10^{-2.95}=0.001122 M](/tpl/images/0548/6523/2ad17.png)
..[1]
![K_a=\frac{[A^-][H^+]}{[HA]}](/tpl/images/0548/6523/a5cb9.png)
![[H^+]=x =0.001122 M](/tpl/images/0548/6523/90707.png)
( from [1])
![pK_a=-\log[K_a]](/tpl/images/0548/6523/78bbf.png)
![=-\log[1.038\times 10^{-5}]=4.98](/tpl/images/0548/6523/44380.png)
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You are given 10.00 mL of a solution of an unknown acid. The pH of this solution is exactly 2.95. Yo...
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