Answer: [tex]4.09\times 10^{-3}[/tex]
Explanation:
Solubility product is defined as the equilibrium constant in which a solid ionic compound is dissolved to produce its ions in solution. It is represented as
The equation for the ionization of the is given as:
[tex]AB\rightarrow A^++B^-[/tex]
Molar concentration = [tex]\frac{moles}{Volume}=\frac{0.0640}{1.00L}=0.0640M[/tex]
By stoichiometry of the reaction:
1 mole of [tex]AB[/tex] gives 1 mole of [tex]A^+[/tex] and 1 mole of [tex]B^-[/tex]
When the solubility of [tex]AB[/tex] is S moles/liter, then the solubility of [tex]A^+[/tex] will be S moles\liter and solubility of [tex]B^-[/tex] will be S moles/liter.
[tex]K_{sp}=[A^{+}][B^{-}][/tex]
[tex]K_{sp}=[0.0640][0.0640]=4.09\times 10^{-3}[/tex]
Thus [tex]K_{sp}[/tex] of the salt at [tex]25^0C[/tex] is [tex]4.09\times 10^{-3}[/tex]
