Which of the following solutions will have highest freezing point?

A. 0.1M KCl
B. 0.05M NaCl
C. 1M AlPO4
D. 0.1MMgSO4 ?
i need it urgently ... pls help...!!!

The highest freezing point will be the one with the smallest delta T and that will occur for the material with the smallest number of particles; i.e., highest van't Hoff factor x molality or i*m

A. 0.1M KCl im = 2*0.1
B. 0.05M NaCl im = 2*0.05
C. 1M AlPO4 im = 1*3
D. 0.1MMgSO4 im = 2*0.1

Thanx a lot DrBob222 :)

Sir, It's MOLARITY (M) not molality (m) given in the question. Do we still have to follow the same formula of i*m...??

0.1MKCL

Ah, freezing point, the temperature at which things start to get a little chilly! Let's see which solution will have the highest freezing point and reign supreme in the cold kingdom.

Now, from the options provided, we have M(KCl), M(NaCl), M(AlPO4), and MM(MgSO4). It's like a tongue-twister, isn't it?

When it comes to freezing point, we're looking for the solute that will disrupt the formation of ice most effectively. The more particles present in a solution, the greater the disruption.

So, let's break it down:

A. 0.1M KCl: One mole of KCl will dissolve into two particles (1K+ and 1Cl-). Therefore, we have 2x0.1 = 0.2 particles.

B. 0.05M NaCl: One mole of NaCl will dissolve into two particles (1Na+ and 1Cl-). Therefore, we have 2x0.05 = 0.1 particles.

C. 1M AlPO4: One mole of AlPO4 will dissolve into four particles (1Al3+, 1PO43-, and 3H2O). Therefore, we have 4x1 = 4 particles.

D. 0.1M MgSO4: One mole of MgSO4 will dissolve into three particles (1Mg2+ and 1SO42-). Therefore, we have 3x0.1 = 0.3 particles.

Now, it's time to crown the champion with the highest freezing point. Since AlPO4 breaks into the highest number of particles, C. 1M AlPO4 takes the icy throne!

So, if you want the highest freezing point, my friend, go with option C and let AlPO4 reign supreme! Stay cool!

To determine which of the given solutions will have the highest freezing point, we need to understand the concept of freezing point depression.

Freezing point depression occurs when a solute is added to a solvent, causing the freezing point of the solvent to decrease. The amount of depression depends on the concentration of the solute particles in the solution.

The freezing point depression formula is given by:

ΔT = Kf * m

Where:
ΔT is the change in freezing point
Kf is the molal freezing point depression constant specific to the solvent
m is the molality of the solution (moles of solute per kilogram of solvent)

The larger the value of m, the lower the freezing point depression.

To determine which of the given solutions will have the highest freezing point, we need to compare the molalities of the solute in each solution.

Let's calculate the molalities of each solution:

A. 0.1M KCl:
The molality is equal to the concentration since 1 mole of KCl is dissolved in 1 kilogram of solvent. Thus, the molality is 0.1M.

B. 0.05M NaCl:
Same as above, the molality is 0.05M.

C. 1M AlPO4:
Since AlPO4 is not a simple ionic compound, we need to calculate its molality using the formula:
molarity = (moles of solute) / (mass of solvent in kg)

Since no information is given about the mass of the solvent, we are unable to calculate the molality accurately. However, based on the given options, it is safe to assume that the molality of AlPO4 would be either equal to or smaller than the molality of KCl or NaCl.

D. 0.1M MgSO4:
Same as option A, the molality is 0.1M.

Comparing the molalities, we can conclude that option A (0.1M KCl) and option D (0.1M MgSO4) have the highest molalities among the given options. Therefore, either option A or option D will have the highest freezing point.