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What is the pH of 0.01 M glycine solutio...

What is the pH of 0.01 M glycine solution? For glycine `K_(a_(1)) = 4.5 xx 10^(-3)` and `Ka_(2) = 1.7 xx 10^(-10)` at 298 K

A

`3.0`

B

`10.0`

C

`6.1`

D

`7.2`

Text Solution

Verified by Experts

The correct Answer is:
D
Glycine `H_(3)N^(+)CH_(2)COO^(-)` is more than basic. Instead of `K_(b)` value , the `K_(a_(2))` value is corresponding to the `k_(b)` value
` :. K_(a) xx K_(b) = 10^(-14)`
` :. ` Overall ionization constant = `K_(a_(1)) xx K_(a_(2))`
`= 4.5 xx 10^(-3) xx 1.7 xx 10^(-10)`
`= 7.65 xx 10^(-13)`
`[H^(+)] =sqrt(K_(a)C)=sqrt(7.65 xx 10^(-13)xx 0.01 )= 8.75 xx 10^(-8) M `
`pH = -log (8.75 xx 10^(-8))`
`= 7.057`
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