5) At what temperature would a 1.55 m NaCl solution freeze, given that the van't Hoff...

Question

Question

5) At what temperature would a 1.55 m NaCl solution freeze, given that the vant Hoff factor for NaCl is 1.9? Kf for water is

Answer 1

Answer #1

AT = ikim ATF - Depression in freering point i vant Hoff factor Kf- Freezing point depression constant ma molality A Tf = 1.

Answer 2

Similar Homework Help Questions

At what temperature would a 1.40 m NaCl solution freeze, given that the van't Hoff factor...

At what temperature would a 1.40 m NaCl solution freeze, given that the van't Hoff factor for NaCl is 1.9? Kf for water is 1.86 ∘C/m . Express your answer with the appropriate units.
You have a aqueous solution of NaCl that has a freezing point of -9.35°C. Assuming a...

You have a aqueous solution of NaCl that has a freezing point of -9.35°C. Assuming a van't Hoff factor of 1.9 for NaCl, what is the mass percent of chloride ion in the solution? (Kf for water is 1.86°C kg/mol).
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute...

Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute. Experimental Results Mass of solvent (water) Freezing point of water Freezing point depression constant (Kf) of water Mass of solution Freezing point of solution 8.515 g 0.00°C 1.86°C/m 9.3589 -5.45°C a. What mass of solute was used? b. What is the...

what is the actual van't hoff factor for an aqueous 0.20 molal solution of FeCl3 if...

what is the actual van't hoff factor for an aqueous 0.20 molal solution of FeCl3 if the freezing point is -1.2C? assume the Kf of water is 1.86C/m
Colligative properties, such as boiling point elevation, depend on the number of dissolved particles in solution....

Colligative properties, such as boiling point elevation, depend on the number of dissolved particles in solution. For nonelectrolytes, no dissociation occurs, and so you can use the number of moles of solute to calculate both molality and molarity. In contrast, electrolytes dissociate, and therefore the molality and molarity must be calculated based on the number of moles of dissociated particles or ions. There are two ions per formula unit of NaCl. Therefore, we would expect the freezing-point depression ΔTf of...
Calculate the osmotic pressure of a 0.0515 M NaCl solution at 25°C. (The van't Hoff factor...

Calculate the osmotic pressure of a 0.0515 M NaCl solution at 25°C. (The van't Hoff factor for NaCl is 1.90)

For an aqueous solution of HF, determine the van't Hoff factor assuming 0% ionization. For the...

For an aqueous solution of HF, determine the van't Hoff factor assuming 0% ionization. For the same solution, determine the van't Hoff factor assuming 100% ionization. A solution is made by dissolving 0.0300 mol HF in 1.00 kg of water. The solution was found to freeze at -0.0644°C. Calculate the value of i and estimate the percent ionization of HF in this solution.
The freezing point depression constant of water is -1.86 C/m. If 7.50 g NaCl is dissolved...

The freezing point depression constant of water is -1.86 C/m. If 7.50 g NaCl is dissolved in 45.0 g H, O, the freezing point is changed by -9.71 *C. Calculate the van't Hoff factor for Naci. Select one: O a. 1,00 . OOOO c. 1.83
Calculate the molality of an aqueous solution of KBr whose freezing point is -4.95 degrees celsius....

Calculate the molality of an aqueous solution of KBr whose freezing point is -4.95 degrees celsius. The Kf of water is 1.86 degrees C/m. Calculate the ideal Van't Hoff factor for KBr? Show work

E GASES, LIQUIDS, AND SOLIDS Calculating and using the van't Hoff factor for electrolytes When 57.5...

E GASES, LIQUIDS, AND SOLIDS Calculating and using the van't Hoff factor for electrolytes When 57.5 g of alanine (CH,NO) are dissolved in 1450. g of a certain mystery liquid X, the freezing point of the solution is 2.1 °C lower than the freezing point of pure X. On the other hand, when 575 g of potassium bromide are dissolved in the same mass of X, the freezing point of the solution is 29 °C lower than the freezing point...