in an aqueous chloride solution cobalt(ii) exists in equilibrium with the complex ion . is pink and is blue. at low temperature the pink color predominates. at high temperature the blue color is strong. if we represent the equilibrium as: we can conclude that:

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06-12-2022
Chemistry

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in an aqueous chloride solution cobalt(ii) exists in equilibrium with the complex ion . is pink and is blue. at low temperature the pink color predominates. at high temperature the blue color is strong. if we represent the equilibrium as: we can conclude that:

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Qwlillyidn Qwlillyidn · Answer 1 · 2022-12-08T09:11:13-05:00

For the given condition, we can conclude that the reaction is an endothermic reaction and to maintain equilibrium the reaction shifts to right side.

Co²⁺(aq) + 4Cl⁻(aq) ⇄ CoCl₄²⁻(aq).

Endothermic reactions are reactions where the reactants absorb heat from its surrounding while the formation of product. These reactions usually reduce the surrounding temperature.

In the given condition it is said that cobalt (ii) exists in equilibrium with complex ion, is blue and pink in color. At low temperature the pink color dominates and at higher temperature, the blue color dominates.

As the given reaction is a reversible reaction, it is easier to maintain the equilibrium. The reaction forms more products in order to maintain the equilibrium. Thus, the reaction absorbs heat and shifts towards right side making the blue color predominant at higher temperature.

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