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Calculate the pH at the equivalence poin...

Calculate the pH at the equivalence point when a solution of 0.1M acetic acid is titrated with a solu- tion of 0.1M NaOH, `K_a` for acid `=2 xx 10^(-5)-`

A

5.7

B

6.7

C

7.7

D

8.7

Text Solution

Verified by Experts

The correct Answer is:
D
Let V ml of acid and V ml of NaOH be used con- centration of both acid and NaOH are same.
`CH_3COOH + NaOH to CH_3COONa + H_2O`
Concentration before reaction `(0.1 xx V)/(2V)=(0.1 xx V)/(2V) 0 " "0`
Concentration after reaction
`0" "0" "(0.1 xx V)/(2V)" "(0.1 xx V)/(2V)`
`[CH_(3)COONa]=(0.1)/(2)=0.05 M`
Now calculate pH by hydrolysis of `CH_(3)COONa CH_(3)COONa+H_(2)O Leftrightarrow CH_(3)COOH+NaOH [OH^(-)]=C.h =sqrt((K_(w).C)/(K_(a))`
`=sqrt((10^(-14) xx 0.05)/(2 xx 10^(-5))`
`=5 xx 10^(-6)`
`p[OH]=6 -0.699=5.301`
`pH=[14-5.301]=8.699 approx 8.7`
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