Question

Write balanced equations and solubility product expressions for the following compounds

Answer 1

Explanation:

Solubility product is defined as the product of the concentrations or solubilities of the ions each raised to the power their stoichiometric coefficients present in the solution. It is expressed as $K_{sp}$.

(a): CuBr

The chemical equation for the dissociation of CuBr into its ions follows:

$CuBr\rightleftharpoons Cu^++Br^-$

The expression of $K_{sp}$ for CuBr follows:

$K_{sp}=[Cu^+][Br^-]$

(b): $ZnC_2O_4$

The chemical equation for the dissociation of $ZnC_2O_4$ into its ions follows:

$ZnC_2O_4\rightleftharpoons Zn^{2+}+C_2O_4^{2-}$

The expression of $K_{sp}$ for $ZnC_2O_4$ follows:

$K_{sp}=[Zn^{2+}][C_2O_4^{2-}]$

(c): $Ag_2CrO_4$

The chemical equation for the dissociation of $Ag_2CrO_4$ into its ions follows:

$Ag_2CrO_4\rightleftharpoons 2Ag^{+}+CrO_4^{2-}$

The expression of $K_{sp}$ for $Ag_2CrO_4$ follows:

$K_{sp}=[Ag^{+}]^2[CrO_4^{2-}]$

(d): $ZnC_2O_4$

The chemical equation for the dissociation of $Hg_2Cl_2$ into its ions follows:

$Hg_2Cl_2\rightleftharpoons 2Hg^{+}+2Cl^{-}$

The expression of $K_{sp}$ for $Hg_2Cl_2$ follows:

$K_{sp}=[Hg^{+}]^2[Cl^{-}]^2$

(e): $AlCl_3$

The chemical equation for the dissociation of $AlCl_3$ into its ions follows:

$AlCl_3\rightleftharpoons Al^{3+}+3Cl^{-}$

The expression of $K_{sp}$ for $AlCl_3$ follows:

$K_{sp}=[Al^{3+}][Cl^{-}]^3$

(f): $ZnC_2O_4$

The chemical equation for the dissociation of $Mn_3(PO_4)_2$ into its ions follows:

$Mn_3(PO_4)_2\rightleftharpoons 3Mn^{2+}+2PO_4^{3-}$

The expression of $K_{sp}$ for $Mn_3(PO_4)_2$ follows:

$K_{sp}=[Mn^{2+}]^3[PO_4^{3-}]^2$