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A 25.0ml sample of 0.1 M HCl is titrated...

A 25.0ml sample of 0.1 M HCl is titrated with 0.1 M NaOH . What is the pH of the solution at the points where 24.9 and 25.1 ml of NaOH have been added ?

A

`3.70,10.70 `

B

` 3.30, 10.30`

C

` 3. 70 , 10 .30`

D

` 3. 0, 11 . 10 `

Text Solution

Verified by Experts

The correct Answer is:
C
` at =24.9 ml`
` N_aV_a =25xx 0.1 , N_b V_b =24.9 xx 0.1`
` [H^(+) ]_("left") =(2.5 - 2.49)/( 50.1 ) =2 xx 10 ^(_4)`
` pOH =3.7 rArr pH =10.3`
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Knowledge Check

  • When a 20 mL of 0.08 M weak base BOH is titrated with 0.08 HCl , the pH of the solution at the end point is 5. What will be the pOH if 10 mL 0.04 M NaOH is added to the resulting solution? [Given : log 2= 0.30 and log 3 = 0. 48 )

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    B
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    C
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    D
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    B
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    D
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  • 20 cc of 'x' M HCl is exactly neutralised by 40 cc of 0.05 M NaOH . The pH of HCl solution is

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    D
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