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Question

Which of the following statements is/are correct about the ionic product of water?

A
At 298K , Equilibrium constant of water < ionic product of water
i.e. Kc<Kw
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B
Kw at 373 K >Kw at 298 K
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C
Ionic product of water at 25C is 1014
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D
None of the above.
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Solution

The correct option is C Ionic product of water at 25C is 1014
Option A : Kc×[H2O]=Kw, we know that concentration of water at 25C or 298K is 100018 M=55.55 MKc<Kw

Option B: Effect of temperature on Kw:

The ionic product of water Kw increases with increase of temperature. The dissociation of water molecule into it's ions is an endothermic reaction.
2H2O(l)H3O+(aq) + OH(aq.)ΔH>0

By Le Chatelier's principle, increase in the temperature will shift the equilibrium in forward direction. So more ions are formed, and Kw increases.
KwT
So, ionic product is greater at 373 K than at 298 K

Option C:
Kw (at 25C)=[H+][OH]=1014

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