Answers: 1
resembles the acid; as a weak acid (a small value of 
) 
would partially dissociate to produce protons 
and 
, its conjugate base. Let the final proton concentration (i.e., ![[H^{+}]](/tpl/images/0083/5038/cab36.png)
) be 
. (Apparently 
) Construct the following RICE table:
![\left\begin{array}{ccc}K_{a}&=&[H^{+}] \cdot [A^{-}] / [HA]\\&=&x^{2} /(0.14 - x)\end{array}\right](/tpl/images/0083/5038/ec898.png)
![\text{pH} = -\text{ln(}[H^{+}]\text{)} / \text{ln(}10\text{)} = 2.1](/tpl/images/0083/5038/74ad5.png)
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If the ka of a monoprotic weak acid is 5.4 × 10-6, what is the ph of a 0.14 m solution of this acid?...
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