Why is the freezing point depresslon of `0.1 M ` NaCl solution nearly twice that of `0.1 M` glocose solution ?

Explanation

NaCl is an electrolyte and it dissociates completely whereas glocose being a non-electrolyte does not dissociate. Hence, the number of particles in `0.1M` NaCl solution is nearly double for NaCl solution than that for glucose solution of same molarity. Therefore depression in freezing point being a colligative property is nearly twice for NaCl solution than that for glucose solution of same molarity.