The freezing point of an aqueous solution depends on the nature and concentration of the solute dissolved in it. When a solute is added to water, the freezing point of the solution decreases compared to that of pure water. The extent of this decrease is directly related to the concentration of the solute particles in the solution.
For equimolar aqueous solutions (meaning they have the same number of moles of solute per liter of solution), the freezing point will be highest for the one with the fewest particles in the solution. This is because the presence of more solute particles will lead to greater depression of the freezing point.
Now, let's compare the given options:
1. Equimolar solution of \(NaCl\) (sodium chloride): This will dissociate into two particles in the solution (\(Na^+\) and \(Cl^-\) ions).
2. Equimolar solution of \(MgCl_2\) (magnesium chloride): This will dissociate into three particles in the solution (\(Mg^{2+}\) and \(2 Cl^-\) ions).
3. Equimolar solution of \(C_6H_{12}O_6\) (glucose): This does not dissociate into ions and remains as individual molecules in solution.
Since the glucose solution does not dissociate and has the fewest particles, it will have the highest freezing point among the equimolar solutions listed. Therefore, the correct answer is the "Equimolar solution of \(C_6H_{12}O_6\) (glucose)." |
