Question: Which Of The Following 0.1 Molar Aqueous Solution Will Have Lowest Freezing Point?

What is Molality formula?

Formulas Needed for Problem Solving The unit of molality is, therefore, expressed in moles per kilogram.

The formula for molality is m = moles of solute / kilograms of solvent..

What is the I in freezing point depression?

ΔTF, the freezing-point depression, is defined as TF (pure solvent) − TF (solution). … b is the molality (moles solute per kilogram of solvent) i is the van ‘t Hoff factor (number of ion particles per individual molecule of solute, e.g. i = 2 for NaCl, 3 for BaCl2).

Which of the following aqueous solution will have highest depression in freezing point?

Since, lowest depression is observed for solution containing urea, hence it will have highest freezing point.

Which of the following aqueous solutions have the lowest freezing point?

Answer and Explanation: The aqueous solution with the lowest freezing point is 1 m MgBr2 , which is choice c. MgBr2 is ionic and soluble and breaks…

Which one has the lowest freezing point?

A 0.01-molar solution of Cu(NO3)2 will have the lowest freezing point. Dissociation of one molecule of cupric nitrate gives 3 ions. All other solutions gives less number of ions. Hence, the depression in freezing point for cupric nitrate is maximum as it gives maximum number of particles in solution.

Which element has highest freezing point?

In the absence of nucleators water can exist as a supercooled liquid down to −48.3 °C (−55 °F, 224.8 K) before freezing. The chemical element with the highest melting point is tungsten, at 3,414 °C (6,177 °F; 3,687 K); this property makes tungsten excellent for use as filaments in light bulbs.

Which of the following 0.1 M aqueous solutions is likely to have the highest depression in freezing point?

Sodium chloride gives two ions and potassium sulphate gives three ions per formula unit. Therefore, the effective number of particles is maximum in potassium sulphate, and it shows the maximum depression in freezing point.

What is molal freezing point?

Kf is the molal freezing point depression constant of the solvent (1.86 °C/m for water). m = molality = moles of solute per kilogram of solvent.

What does freezing point depend on?

The freezing point of the solvent in a solution changes as the concentration of the solute in the solution changes (but it does not depend on the identity of either the solvent or the solute(s) particles (kind, size or charge) in the solution).

Why does solute lower freezing point?

The introduction of a solute reduces the activity of the liquid phase solvent, thereby reducing the rate of freezing. You can think of this reduction in activity as solute molecules “getting in the way” of solvent molecules from attaining the correct alignment for freezing at the surface.