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The chemical reaction [Zn(OH)2(s) ←→ Zn2+(aq) + 2OH- (aq) 1. Why did you add more 1M...

The chemical reaction

[Zn(OH)2(s) ←→ Zn2+(aq) + 2OH- (aq)

1. Why did you add more 1M naOH solution to your test tube? Using LeChateliers principle, explain how the NaOH shifted the equilibrium between [Zn(OH)2(s) ←→ Zn2+(aq) + 2OH- (aq). Explain how the equilibrium system responded to counteract the change.

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Answer #1

1) The addition of 1M NaOH will increase the concentration of [OH-] in the reaction, leading to the value of Qc>Kc, in order to reach the same value of Kc, the reaction will move in the reverse direction (i.e. products concentration will decrease and the reaction concentration will increase in the reaction)

The equilibrium will counteract the change by establishing the reaction in reverse direction, which will lead to the increase in the concentration of Zn(OH)2 and reduction in the concentration of both Zn(+2) and 2OH(-)

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