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Q.

20 mL of 0.1 M acetic acid is mixed in a solution of NaOH. If 10 mL of 0.1 M NaOH is present in then H+  concentration in resulting solution is (Ka of  acetic = 1.7 × 10–5)

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a

1.7 \times {10^{ - 2}}

b

1.7 \times {10^{ - 5}}

c

\large 3.4 \times {10^{ - 5}}

d

1.7 \times {10^{ - 7}}

answer is C.

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Detailed Solution

Following reaction will occur

  CH3COOH +NaOH → CH3COONa + H2O
t = 0 0.1 x 20 = 2, 0.1 x 10 = 1       0
\large t = t_\infty 2 - 1 = 1      , 1 - 1 = 0       1

Resultant solution is an acidic buffer. Such a soltuion has a PH given as.

\large {P^H} = {P^{{K_a}}} + \log \frac{{\left[ {salt} \right]}}{{\left[ {acid} \right]}}

\large \Rightarrow {P^H} = 4.74 + \log \frac{1}{1} = 4.74

\large \Rightarrow \left[ {{H^ + }} \right] = 1.7 \times {10^{ - 5}}

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