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-)]`

Step-by-step 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-)]`