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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))=4.5xx10^(-3)` and `K_(a_(2))=1.7xx10^(-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:
C
Glycine `H_(3)N^(+)CH_(2)CO O^(-)` is more acidic than basic. Instead of `K_(b)` value, the second given `K_(a)` value is corresponding to the `K_(b)` value `(.:' K_(a)xxK_(b)=10^(-14))`.Hence, overall ionization constant,
`K_(a_(1))xxK_(a_(2))=4.5xx10^(-3)xx1.7xx10^(-10)`
`=7.65xx10^(-13)`
`[H^(+)]=sqrt(KC)=sqrt(7.65xx10^(-13)xx0.01)`
`=sqrt(0.765xx10^(-14))=0.87xx10^(-7)M`
`pH = - log (0.87xx10^(-7))=7-0.93=6.07`
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Knowledge Check

  • 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

  • What is the pH of 10^(-3) M ammonia cyanide solution, if K_(HCN)=7.2 xx 10^(-11) and K_(NH_(3))=1.8 xx 10^(-5)mol L^(-1) ?

    A
    14
    B
    9.7
    C
    `12.0`
    D
    `7.5`

  • The pH of a 0.1 M solution of NH_(4)OH (having K_(b)=1.0xx10^(-5)) is equal to

    A
    10
    B
    6
    C
    11
    D
    12

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