Question

Consider the equilibrium describing the endothermic dissolution of a solid in water. Z n ( O H ) 2 ( s ) − ⇀ ↽ − Z n 2 + ( a q ) + 2 O H − ( a q ) If you have a saturated solution at equilibrium, what changes could you make to increase the solubility of the compound? g

Answer 1

Answer:

- Add more zinc hydroxide.

- Increase the temperature.

Explanation:

Hello,

Based on the given chemical reaction at equilibrium:

$Z n ( O H )_ 2 ( s ) \rightleftharpoons Z n ^{2 +} ( a q ) + 2 O H ^- ( a q )$

Thus, by considering the Le Chatelier's principle, increasing the zinc hydroxide solubility, it means favor the direct reaction, could be attained by:

- Adding more zinc hydroxide as the addition of products favor the formation of products.

- As the reaction is endothermic, the energy is considered as a reactant, therefore, increasing the temperature the direct reaction is favored.

Best regards.