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The solubility product (K(sp)) of Ca(OH)...

The solubility product (`K_(sp)`) of `Ca(OH)_(2)` at `25^@` is `4.42xx10^(-5)`. A 500 mL of saturated solution of `Ca(OH)_(2)` is mixed with equal volume of 0.4 M NaOH. How much `Ca(OH)_(2)` in milligrams is precipitated?
At equilibrium, the solution contains 0.0358 mole of `K_(2)CO_(3)`. Assuming the degree of dissociation of `K_(2)C_(2)O_(4)` and `K_(2)CO_(3)` to be equal, calculate the solubility product of `Ag_(2)CO_(3)`.

Text Solution

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`817.7 `mg
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The K_(sp) of Ca(OH)_(2) is 4.42 xx 10^(-5) at 25^(@)C . A 500 ml of saturated solution of Ca(OH)_(2) is mixed with an equal volume of 0.4M NaOH . How much Ca(OH)_(2) in mg is precipitated ?

The K_(SP)of Ca(OH)_(2)is 4.42xx10^(-5)at 25^(@)C . A 500 mL of saturated solution of Ca(OH)_(2) is mixed with equal volume of 0.4M NaOH . How much Ca(OH)_(2) in mg is preciptated ?

Knowledge Check

  • The solubility product of Ca(OH)_(2) at 250^(0)C is 4.42 xx 10^(-5) . A 500 mL of saturated solution of Ca(OH)_(2) is mixed with equal volume of 0.4 M NaOH . How much Ca(OH)_(2) on milligram is precipitated?

    A
    `758.2mg`
    B
    `725.2 mg`
    C
    `785.2 mg`
    D
    `658.2 mg`

  • pH of a saturated solution of Ba(OH)_(2) is 12. The value of solubility product (K_(sp)) of Ba(OH)_(2) is

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    B
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    C
    `4.0 xx 10^(-6)`
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    The K_(sp) of Ca(OH)_(2) is 4.42xx10^(-5) at 25^(@)C . 500 mL of saturated solution of Ca(OH)_(2) is mixed with equal volume of 0.4 M NaOH . How much Ca(OH)_(2) in mg will be precipitated ? Also calculate percentage precipitation.

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