From your predicted the value of the van't Hoff factor, calculate the boiling point of a 1.58 m aqueous solution of barium nitrate, Ba(NO3)2? The Kb of water is 0.52°C/m.
From your predicted the value of the van't Hoff factor, calculate the boiling point of a...
The boiling point of an aqueous 3.0M ethylene glycol (C2H6O2) solution is 102oC and the freezing point is-10.8oC. What is the experimental van't Hoff factor (i) and how does it compare to the theoretical van't Hoff factor?
van't Hoff Factor Chem 202 Freezing Point of Aqueous Solutions Results Experimental freezing point values determined from graphs (sce directions on p. 3-5, steps 2,3): Sample Ty measured /°C AT measured / °C Distilled Water (solvent) -0.1°C Follow your instructor's Solution D (Naci) -1.8°C 1.7°C directions for submitting these values Solution G (lalla) -1.0°C 0.9°C before you leave lab! van't Hoff factor values (see directions on p. 3-6, steps 4-5): Solution D Solute Compound Naci Molality 0.505 mol/kg Ideal van't...
Calculate the molality and van't Hoff factor (i) for the following aqueous solution: 0.775 mass % KCl, freezing point = −0.364°C m = m KCl i =
Calculate the molality and van't Hoff factor (i) for the following aqueous solution: 2.460 mass % H2SO4, freezing point = −1.056°C m = m H2SO4? i = ?
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.
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 the freezing point is -1.2C? assume the Kf of water is 1.86C/m
Solutes do not typically exhibit ideal behavior in solution, resulting in non-integer van't Hoff factors. Based on this information, which of the following solutes is most likely present in a 2.12 m aqueous solution with a boiling point of 103.87°C? (Kb for water is 0.512°C/m) NaBr C6H12O6 Na3PO4 Ca(ClO3)2
The boiling point of an aqueous 1.83 m (NH4)2SO4 (molar mass = 132.15 g/mol) solution is 102.5°C. Determine the value of the van't Hoff factor for this solute if the Kb for water is 0.512°C/m. Answer's 2.7 but I have no idea how to solve for this, can someone show me how to solve with LOTS of steps? Thanks.
1. What is the expected van't Hoff factor for FeCl3? (Assume dilute conditions) A) 1 B) 2 D) 4 C) 3 E) 5 2. Choose the aqueous solution that has the highest boiling point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. A) 0.100 mol kg-1 NaCl B) 0.100 mol kg-1 AlCl3 C) 0.100 mol kg-1 MgCl2 D) 0.100 mol kg-1 C6H1206 E) They all have the same boiling point.