Why on dilution the Λm of CH3COOH increases drastically, while that of CH3COONa increases gradually?
Why on dilution the Λm of CH3COOH increases drastically, while that of CH3COONa increases gradually?
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In the case of CH3COOH, which is a weak electrolyte, the number of ions increase on dilution due to an increase in degree of dissociation.
CH3COOH + H2O CH3COO— + H3O+
In the case of strong electrolyte the number of ions remains the same but the interionic attraction decreases.
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