Answer : The molar solubility of [tex]C_2d_3[/tex] is [tex]9.67\times 10^{-3}M[/tex]
Explanation :
The solubility equilibrium reaction will be:
[tex]C_2d_3\rightleftharpoons 2C^{3+}+3d^{2-}[/tex]
The expression for solubility constant for this reaction will be,
Let the molar solubility be, 'x'
[tex]K_{sp}=(2x)^2\times (3x)^3[/tex]
Now put all the given values in this expression, we get:
[tex]9.14\times 10^{-9}=108x^5[/tex]
[tex]x=9.67\times 10^{-3}M[/tex]
Therefore, the molar solubility of [tex]C_2d_3[/tex] is [tex]9.67\times 10^{-3}M[/tex]
