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What is the concentration of CN^(-) ion...

What is the concentration of `CN^(-) ` ions in a solution with 0.1 M HCl and 0.01 M HCN where `K_a` of HCN is `10 ^(-6) ` ?

A

`[H^(+) ]_("total") ~~[H^(+) ]` from first step ionization of acid `H_2A `

B

Concentration of `OH^(-) ` in solution is `10 ^(-3) ` M

C

The value of `K_(a_1) ` is nearly `10 ^(5)`

D

` p^(ka_2) - p^(ka_1) =9`

Text Solution

Verified by Experts

The correct Answer is:
A, C
` [H^(+) ]=sqrt(K_(a_1) xx C ) rArr 10^(-3) =sqrt( K_(a_1)xx 10^(-1)) `
` K_(a_1) =10 ^(-5) rArr [A^(-2) ]=K_(a_2) rArr P^(K_(a2 )) = 12 `
` P^(K_(a2)) -P^(K_(a3)) = 7 `
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Knowledge Check

  • What is the maximum concentration of Mg^(+2) that can be introduced into a solution containing 0.1 M NH_3 and 0.01 M NH_4^(+ ) without causing precipitation of Mg (OH)_2 ? K_b of NH_3 = 10^(6) K_(sp) of Mg(OH)_2 =1.2 xx 10^(-12)

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    ` 0.012 M`
    B
    ` 0.24 M`
    C
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    D
    ` 0.048 M`

  • What is the [CN^(-)] in a solution prepared by mixing 100ml 0.1IM KCN and 100ml 0.2M HCI? (K_(x) " of " HCN = 5 xx 10^(-6) )

    A
    `5 xx 10^(-4)` M
    B
    `2 xx 10^(-6)` M
    C
    `5 xx 10^(-6)` M
    D
    `2 xx 10^(-5)` M

  • The weak acids undergo partial ionisation is aqueous medium. However the dissociation of weak acids is suppressed by presence of common ions. But the Ka value of the acid remains constant irrespective of extent of dissociation What is [CN^(-)] J in a solution prepared by mixing 100ml 0.1M KCN and 100 ml 0.1 M HCl ? (K_(a) of HCN= 5xx 10^(-6) )

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    B
    `2 xx 10^(-6)` M
    C
    `2 xx 10^(-5)` M
    D
    `4 xx 10^(-6)` M

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