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Find the solubility product of a saturat...

Find the solubility product of a saturated solution of `Ag_(2)CrO_(4)` in water at `298K`, if the `EMF` of the cell `:`
`Ag|Ag^(o+)(satAg_(2)CrO_(4)sol)||Ag(0.1M)|Agis 0.164V` at `298K`.

Text Solution

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The correct Answer is:
`K_(sp) = 2.287 xx 10^(-12)`
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The expression for the solubility product of Ag_(2)CrO_(3) will be

The [Ag^(+)] ion in a saturated solution of Ag_(2)CrO_(4) at 25^(@)C is 1.5xx10^(-4)M . Determine K_(SP) of Ag_(2)CrO_(4) at 25^(@)C .

What is the solubility of Ag_(2)CrO_(4) in water if the value of the solubility product (K_(sp))=1.3 xx 10^(-11) (mol//L)^(3) ?

Which is the correct representation for the solubility product constant of Ag_(2)CrO_(4) ?

Knowledge Check

  • The expression for the solubility product of Ag_(2)CrO_(3) will be

    A
    `K_(sp) = S^(2)`
    B
    `K_(sp) = 4S^(3)`
    C
    `K_(sp) = 27S^(4)`
    D
    `K_(sp) = S`

  • Which is the correct representation of the solubility product constant of Ag_(2)CrO_(4)

    A
    `[Ag^(+)]^(2)[CrO_(4)^(-2)]`
    B
    `[Ag^(+)] [CrO_(4)^(-2)]`
    C
    `[2Ag^(+)] [CrO_(4)^(-2)]`
    D
    `[2Ag^(+)]^(2) [CrO_(4)^(-2)]`

  • The e.f.m. of the cell Ag|Ag^(+)(0.1M)||Ag^(+)(1M)|Ag at 298K is

    A
    0.0059V
    B
    0.059V
    C
    5.9V
    D
    0.59V
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