When solid calcium chloride was added (tubes 3 and 4), the equilibrium shifted t

Question

When solid calcium chloride was added (tubes 3 and 4), the equilibrium shifted toward the left side. When solid calcium nitrate was added (tube 5) no change in equilibrium position was observed. How do you explain these observations? Based on the information provided, which ion was removed from the equilibrium system upon addition of silver nitrate (tube 4)? Did removal of the ion cause the equilibrium to shift toward the left or right side? How do you know? The equilibrium system of cobalt(II) complex is highly exothermic. Does increasing or decreasing the reaction temperature cause the equilibrium to shift toward the right side (the water complex)? How do you know? Which reaction conditions will make the formation of a cobalt(III) complex with chloride as complete as possible?

Explanation / Answer

Based on these question, the equilibrium may be,

[CoCl4]2- (aq.) + 4 H2O (l) = [Co(H2O)4]2+ (aq.) + 4 Cl- (aq.)

(11) SInce the Cl- ions are right side, addition of CaCl2 solid to this equilibrium mixture, increase the concentration of Cl- ion, which causes to shift the equilibrium towards left side.

CaCl2 (aq.) -------> Ca2+ (aq.) + 2 Cl- (aq.)

But addtion of solid calcium nitrate does not affect the cocnetration of any ion at equilibrium.

Ca(NO3)2 (aq.) ---------> Ca2+ (aq.) + 2 NO3- (aq.)

(12)

Upon addition of AgNO3 solution the chloride ions will be removed as the AgCl precipitate.

AgNO3 (aq.) + Cl- (aq.) --------> AgCl (s) + NO3- (aq.)

Due to this reaction, theconcentration of Cl- ions will decrease, which causes to shift the equilibrium towards right side.

(13)

Since the equilibrium system is exothermic in nature (i.e. forward is exothermic in nature), decrease in temperature will favor the forward reaction i.e towards the water equilibrium complex.

(14)

That is to maximum shift the equilibrium towards left side,

(i) Increase in concentration of Cl- i.e additon of CaCl2 shifts towards left side.

(ii) Increase in temperature as it favors endothermic i.e backward in the present case.

(iii) Removal of cobalt chloride complex formed.

These condition will favour tho form cobalt chloride complex.

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