Why does 1 mol of CaCl2 lower the freezing point of water more than 1 mol of Nacl
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this happens because salt completely dissociates in aquous solution , while suger does not . This aspect is important when dealing with colligative property because the number of particles will differ for the aforementioned compounds.
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1 mol of CaCl2 lowers the freezing point of water more than 1 mol of NaCl because it forms more ions on dissociating as compared to NaCl.
- The dissociation of CaCl2 can be given as:
CaCl2 ⇄ Ca²⁺ + 2 Cl⁻
- The dissociation of NaCl can be given as:
NaCl ⇄ Na⁺ + Cl⁻
- The depression in freezing point is a colligative property, i.e., it depends upon the no of particles of solute.
- SInce CaCl2 dissociates to form 3 ions, it will lower the freezing point of water more as compared to NaCl which forms only 2 ions on dissociation.
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