Question

What is the correct formula for the Ksp of the reaction Cu2CO3 (s) mc027-1.jpg 2Cu+ (aq) + CO3 2– (aq)? Ksp = [Cu+ ][CO3 2– ] Ksp = [Cu+ ][CO3 2– ]2 Ksp = 2[Cu+ ][CO3 2– ] Ksp = [Cu+ ]2 [CO3 2– ]

Answer 1

Ksp = [Cu^+]^2 [CO3^2-]

Answer 2

Answer: $K_{sp}=[Cu^+]^2[CO_3^{2-}]$

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 $K_{sp}$

The equation for the ionization of the given compound is given as:

$Cu_2CO_3\leftrightharpoons 2Cu^{+}+CO_3^{2-}$

By stoichiometry of the reaction:

1 mole of $Cu_2CO_3$ gives 2 moles of $Cu^{+}$ and 1 mole of $CO_3^{2-}$.

When the solubility of $Cu_2CO_3$ is S moles/liter, then the solubility of $Cu^{+}$ will be 2S moles\liter and solubility of $CO_3^{2-}$ will be S moles/liter.

Expression for the equilibrium constant of $Ag_2CrO_4$ will be:

$K_{sp}=[Cu^+]^2[CO_3^{2-}]$