The solubility product of a salt having general formulaMX_{2} in water is 4 \times 10^{-12}. The concentration of M^{2+} ions in the aqueous solution of the salt is

  • Option 1)

    2.0\times 10^{-6}M

  • Option 2)

    1.0\times 10^{-4}M

  • Option 3)

    1.6\times 10^{-4}M

  • Option 4)

    4.0\times 10^{-10}M

 

Answers (1)

As we learnt in 

General expression of solubility product -

M_{x}X_{y}\rightleftharpoons xM^{p+}(aq)+yX^{2-}(aq)


(x.p^{+}=y.\bar{q})

- wherein

Its solubility product is 
 

K_{sp}=[M^{p+}]^{x}\:[X^{2-}]^{y}

 

K_{sp}=s\; .\; (2s)^{2}=4s^{3}

4\times 10^{-12}=4s^{3}\; or\; s^{3}=1\times 10^{-12}

or\; \; s=1\times 10^{-4}M\Rightarrow \left [ M^{2+} \right ]=1\times 10^{-4}M


Option 1)

2.0\times 10^{-6}M

This option is incorrect

Option 2)

1.0\times 10^{-4}M

This option is correct

Option 3)

1.6\times 10^{-4}M

This option is incorrect

Option 4)

4.0\times 10^{-10}M

This option is incorrect

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