If a 0.750 ? aqueous solution freezes at −2.80 ∘C, what is the van't Hoff factor, ?, of the solute? Consult the table of ? f values.
If a 0.750 ? aqueous solution freezes at −2.80 ∘C, what is the van't Hoff factor,...
lf a 0.880 m aqueous solution freezes at-3.50 °C, what is the van't Hoff factor, і, of the solute? Kt values can be found here. Number
If an 0.860 m aqueous solution freezes at –2.10 °C, what is the van\'t Hoff factor, i, of the solute? Kf values can be found here.
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...
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.
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
-4 (3 pts.) If a 0.830 m aqueous solution freezes at -3.58 °C, what is the van't Hoff factor, i, of the solute? On Blackboard, please enter your response as a number with three significant figures le X.XX where the X's are numbers). Please do not use exponent notation or fractions. Also, please write your answer in the box.
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...
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?
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 = ?