Calculate [H+] of solution obtained by mixing equal volume of 0.02 M H – InterviewSolution

1.	Calculate [H+] of solution obtained by mixing equal volume of 0.02 M HNO2 ( a weak acid) and 0.2 M CH3COOH solution. Given that: Ka1(HNO2)=2×10−4 Ka2(CH3COOH)=2×10−5 Where , Ka1and Ka2 are the dissociation constants of HNO2 and CH3COOH respectively.
Answer» Calculate $[H^{+}]$ of solution obtained by mixing equal volume of 0.02 M $H N O_{2}$ ( a weak acid) and 0.2 M $C H_{3} C O O H$ solution. Given that: $K_{a_{1}} (H N O_{2}) = 2 \times 10^{- 4}$ $K_{a_{2}} (C H_{3} C O O H) = 2 \times 10^{- 5}$ Where , $K_{a_{1}} a n d K_{a_{2}}$ are the dissociation constants of $H N O_{2} a n d C H_{3} C O O H$ respectively.

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