A solution (in this experiment solution of NaNO₃) freezes at a lower temperature than does the pure solvent (deionized water). The higher the
solute concentration (sodium nitrate), freezing point depression of the solution will be greater. Equation describing the change in freezing point: ΔT = Kf · b · i. ΔT - temperature change from pure solvent to solution. Kf - the molal freezing point depression constant. b - molality (moles of solute per kilogram of solvent). i - Van’t Hoff Factor. First measure freezing point of pure solvent (deionized water). Than make solutions of NaNO₃ with different molality and measure separately their freezing points. Use equation to calculate Kf.
The answer is atomic radii; the size or radii of an atom increases from left to right, versus the ionization energies and electronegativities of atoms which increase from right to left.
