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Equilibrium
Question
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Explain why pure liquids and solids can be ignored while writing the equilibrium constant expression?

Answer

The concentration of pure liquids and solids in the equilibrium expression for heterogeneous reactions are ignored because their concentrations remain constant. By convention, the concentration of all pure solids and pure liquids is taken as unity, i.e.
[solid] = 1, [liquid] = 1.

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Some More Questions From Equilibrium Chapter

Which measurable property becomes constant in water vapour equilibrium?

Give an example from daily life in which there is gas solution equilibrium?

A crystal of common salt of a given mass is kept in its aqueous solution. After 24 hours, its mass remains the same. Is the crystal in equilibrium with the solution?

What is the role of forward and backward reactions at equilibrium of a reversible reaction?

What is a forward reaction?

What condition favours a reversible reaction?

What is a backward reaction?