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What is the pH of the resulting solution...

What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?

A

2

B

7

C

1.04

D

12.65

Text Solution

Verified by Experts

The correct Answer is:
D
One mole of NaOH is completely neutralised by one mole of HCl. Hence, 0.01 mole of NaOH will be completely neutralised by 0.01 mole of HCl.
NaOH left unneutralised =0.1-0.01 mol =0.09 mol. As equal volumes of two solutions are mixed.
`[OH]^- =(0.09)/2=0.045 M rArr pOH =-log (0.045)=1.35`
`pH =14-1.35=12.65`
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