Which of the following will have the highest freezing point 1M urea?

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

Why is osmotic pressure of 1M KCl is higher than 1M urea solution?

Answer: Osmotic pressure of 1 m higher than 1 m urea solution as osmotic pressure is a colligative property which depends on the amount of solute. Thus the number of moles will be more on addition of KCl and lesser number of moles on addition of urea.

Which of the following has highest freezing point 1M NaCl?

glucose
Greater the value of n, greater is the van’t hoff factor. The lowest van’t hoff factor will result in the least depression in freezing point and hence that solution will have the highest freezing point. Hence, the correct option is D, glucose.

Which solution has highest freezing?

(a) 1M glucose solution has highest freezing point because it has lowest ΔTf.

What is the osmotic pressure of KCl?

50 atmospheres
The osmotic pressure of a potassium chloride solution (at 300K) is 50 atmospheres.

Which of the following solution has highest osmotic pressure 1M NaCl?

NaCl gives maximum number of ions hence it will show highest osmotic pressure.

Which of these has the highest freezing point a 1M glucose B 1M NaCl C 1M CaCl2?

Explanation: glucose solution has highest freezing point bcause it has lowest delta Tf (the change in freezing point).

Which one has higher freezing point KCl or 1m urea solution?

Out of 1M urea solution and 1MKCl solution, which one has higher freezing point? Freezing point depends on Van’t Hoff factor (i). Thus KCl has highest freezing point. Was this answer helpful?

What is the molarity of solute particles in 1 M urea?

Now urea does not dissociate so the molarity of solute particles in 1 M urea is in fact just 1.0 M, so that this solution would freeze at about 1.9 deg-C less than pure water.

What is the molarity of 1 M KCl?

On the other hand, KCl dissociates into K+ and Cl- ions, so that a 1 M KCl solution would be approximately 2.0 M in solute particles, and the freezing point should be about 3.8 deg-C less than that of pure water. Often molality (the number of moles solute per kg of solvent) is used in place of molarity (the number of moles solute per L solution).

How many molar solutions of glucose phenol and potassium chloride were prepared?

0.01 molar solutions of glucose, phenol and potassium chloride were prepared in water. The boiling points of Which of the following has minimum freezing point [Pb. PMT 1999] Please Wait you are being redirected….