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100 ml of 0.1 M HCl and 100 ml of 0.1 M ...

100 ml of 0.1 M HCl and 100 ml of 0.1 M HOCN are mixed . What is the concentration of `.. OCN ^(-)..`, and pH of the solution ? ` (K_a=1.2 xx 10^(-6) ) `

A

` 1.2 xx 10^(-6) , 1.3 `

B

` 1.2 xx 10^(-6) ,1`

C

` 2.6 xx 10^(-8) ,1.6`

D

` 2.4 xx 10^(-6) , 2.6`

Text Solution

Verified by Experts

The correct Answer is:
A
`[H^(+)]= (100 xx 0.1 )/( 200) =0.05,pH =2- log 5 =13`
` [HOCN]=( 100xx 0.1 )/( 200) = 0.05`
` K_a =([H^(+) ][OCN^(-) ])/( [HOCN]) =(1.2 xx 10 ^(-6) xx 0.05 )/( 0.05 ) `
` = [OCN^(-) ]=1.2 xx 10^(-6) `
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Knowledge Check

  • 100 ml of 0.1 M HCl and 100 ml of 0.1 M HOCN are mixed then (K_a= 1.2 xx 10^(-6))

    A
    `OCN^(-) ` concentration in the solution is `1.2 xx10^(-6) `
    B
    pH of the solution is 1.3
    C
    solution is a buffer
    D
    `H^(+) ` in the solution is `10^(6) `

  • 100 ml of 0.1 M HCl and 100 ml of 0.1 M HOCN are mixed then (K_a= 1.2 xx 10^(-6))

    A
    `OCN^(-) ` concentration in the solution is `1.2 xx10^(-6) `
    B
    pH of the solution is 1.3
    C
    solution is a buffer
    D
    `H^(+) ` in the solution is `10^(6) `

  • 100 ml of 0.1 M HCI and 100 ml of 0.1 M HOCN are mixed then (K_(a), = 1.2 xx 10^(-6) )

    A
    `OCN^(-)` concentration in the solution is `1.2 xx 10^(-6)`
    B
    pH of the solution is 1.3
    C
    solution is a buffer
    D
    `H^(+)` in the solution is `10^(-6)`

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