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The hydrolysis constang of 0.1M aqueous ...

The hydrolysis constang of `0.1M` aqueous solution of sodium acetate if `K_(a)` of `CH_(3)COOH = 1.8 xx 10^(-5)` is

A

0.556

B

4.72

C

9.38

D

5.56

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A
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Knowledge Check

  • What is the pH of an aqueous solution of an acetate ( K_a = K_b = 1.8 xx 10^(-5) )

    A
    `gt 7`
    B
    7
    C
    `lt 7.0`
    D
    Zero

  • What is the pH of an aqueous solution of ammonium acetate (K_a= K_b =1.8 xx 10^(-5))

    A
    `gt 7`
    B
    7
    C
    `lt 7.0`
    D
    Zero

  • What will be the hydrogen ion concentration of a solution obtained by mixing 500ml of 0.2 M acetic acid and 500ml of 0.4 M sodium acetate ? (K_(a)CH_(3)COOH)=1.8 xx 10^(-5))

    A
    `1.8 xx 10^(-5)`
    B
    `0.9 xx 10^(-6)`
    C
    `9 xx 10^(-6)`
    D
    `1.6 xx 10^(-4)`

    • Similar Questions

    Explore conceptually related problems

    Calculate the pH of a 0.01 N solution of acetic acid. K_(a) for CH_(3)CO OH is 1.8xx10^(-5) at 25^(@) C.

    Calculate the percentage hydrolysis of decinormal solution of ammonium acetate given that k_(a) = 1.75 xx 10^(-5), K_(b) =1.80 xx 10^(-5) and K_(w) = 1.0 xx 10^(-14)

    Calculate the degree of hydrolysis of a decimolar solution of ammonium acetate at 25^@C . K_a(CH_3COOH)=1.75xx10^(-5), K_b(NH_4OH)=1.81xx10^(-5)

    a. Calculate the percentage hydrolysis of 0.003M aqueous solution of NaOH. K_(a) for HOCN = 3.3 xx 10^(-4) . b. What is the pH and [overset(Theta)OH] of 0.02M aqueous solution of sodium butyrate. (K_(a) = 2.0 xx 10^(-5)) .

    Calculate pH solution: 0.1 M CH_(3)COOH (K_a=1.8 xx 10^(-5))

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