The solubility of a salt of weak acid (AB) at pH 3 is `Y xx 10^(-3) " mol "L^(-1)`. The value of Y is ____. (Given that the value of solubility product of AB `(K_(sp))=2xx10^(-10)` and the value of ionization constant of HB `(K_(a))=1xx10^(-8)`)
Text Solution
Verified by Experts
The correct Answer is:
4.47
`S = sqrt(K_(sp)(([H^(+)])/(K_(a))+1)) = sqrt(2 xx10^(-10)((10^(-3))/(10^(-8))+1)) = sqrt(2 xx 10^(-5))` `= 4.47 xx 10^(-3) M`
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Knowledge Check
If the solubility of MX_(2) ( a sparingly soluble salt is 2.5 xx 10^(-4) mol^(-1) . The value of K_(sp) of the salt would be
A
`6.25 xx 10^(-11)`
B
`12.5 xx 10^(-8)`
C
`6.25 xx 10^(-8)`
D
`3.125 xx 10^(-11)`
The solubility of a springly soluble salt AB_(2) in water is 1.0xx10^(-5) mol L^(-1) . Its solubility product is:
A
`10^(-15)`
B
`10^(-10)`
C
`4xx10^(-15)`
D
`4xx10^(-10)`
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