Question

Consider the following system at equilibrium. CaCO3(s) Double headed arrow. Ca2 (aq) CO32â€""(aq) The addition of which compound will cause a shift in equilibrium because of a common ion effect? CCl4 CO2 CuSO4 Na2CO3.

Answer 1

The compound that has been capable to shift the equilibrium with common ion effect has been  $\rm \bold{Na_2CO_3}$.  Thus, option D is correct.

The complete equation for the decomposition of calcium carbonate has been:

$\rm CaCO_3\rightleftharpoons Ca^2^+\;+\;CO_3^2^-$

The equilibrium has been the state in the reaction, when the number of products and has been equivalent to the number of reactants. The increase or decrease in the concentration of any of the reactant or product results in the shift in the equilibrium.

For the given reaction, the addition of Calcium or carbonate ions to the solution results in the increase in the product concentration with the common ion effect, and thereby shifts the equilibrium condition.

The ions liberated by the following compounds has been:

$\rm CCl_4\;=\text{not dissolved}\\CO_2\;+\;H_2O\leftrightharpoons CO_3^-\;+\;H^+\\CuSO_4\leftrightharpoons Cu^2^+\;+\;SO_4^2^-\\Na_2CO_3\leftrightharpoons 2\;Na^+\;+\;CO_3^-$

The compound, that has been capable of liberating the carbonate ions in the medium has been $\rm \bold{Na_2CO_3}$. Thus, it results in the shift of the equilibrium due to common ion effect. Hence, option D is correct.

For more information about common ion effect, refer to the link:

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