Moving to another question will save this response. stion 13 A 11.44 gram sample of a compound with a molar mass of 124.0 g mol~1, when dissolved in 112.9 g of water, gave a solution which had a freezing point -1.46 "C. Calculate the experimental value of the van't Hoff factor. Kf for water = 1.86 °C m-1 (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 12.3 and 123 and 123.) MQuestion 13 of 29

Moving to another question will save this response. stion 13 A 11.44 gram sample of a compound with a molar mass of 124.0 g mol~1, when dissolved in 112.9 g of water, gave a solution which had a freezing point -1.46 "C. Calculate the experimental value of the van't Hoff factor. Kf for water = 1.86 °C m-1 (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 12.3 and 123 and 123.) MQuestion 13 of 29

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

When 0.6 g of sample of an unknown substance (assume the van t'Hoff factor =1) are dissolved in 11.9 g of camphor (with Kf = 39.7°C/m) its freezing point decreases by 3.02°C. What is the molar mass of unknown substance (in g/mol)? Give your answers to three sig figs
What mass of glucose (molar mass 180.16 g/mol, i=1) must be dissolved in 2.50 kg of solvent to lower the freezing point by 0.500 oC if the freezing point depression constant of the solvent is 9.51 oC/m?
PLease don't provide hand writtin solution...
When 45.1 g of benzamlde (C,H,NO are dissolved In 850. g of a certaln mystery liquld X, the freezing point of the solutlon Is 7.70 °C less than the freezing polnt of pure X. that must be dissolved In the same mass of X to produce the same depression In freezing point. The van't 3/3) Calculate the mass of Iron(III) nitrate (Fe(NO. Hoff factor i=3.48 for Iron(III) nitrate in X. do Be sure your answer has a unit symbol, if necessary, and Is rounded to the correct number of significant digits. x10 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibi Check Explanation M 9 hp 火

When 0.253 g of benzoic acid, C6H5COOH, is dissolved in 12.45 g of cyclohexanol, C6H11OH, thefreezing point of cyclohexanol is lowered by 6.55oC. What is the molal freezing point depressionconstant, Kf, for this solvent? Show all calculations.
A 0.5 M NaOH solution has a density of 1.0295 g/mL. Calculate the w% and the molality of the 0.5 M NaOH solution.
When 319. g of glycine (C₂H, NO₂) are dissolved in 1250. g of a certain mystery liquid X, the freezing point of the solution is 2.10 °C less than the freezing point of pure X. Calculate the mass of sodium chloride that must be dissolved in the same mass of .X to produce the same depression in freezing point. The van't Hoff factor i=1.70 for sodium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits. 0 0.0 8 X 2
Please don't provide hand writttin solution...
Answer the attached photo.
When 205. g of benzamide (C,H,NO) are dissolved in 550. g of a certain mystery liquid X, the freezing point of the solution is 2.50 °C less than the freezing point of pure X Calculate the mass of iron(111) nitrate (Fe(NO₂),) that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor i-3.44 for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits. 10 of 0 0.0 cla 0.2 A
The boiling temperature of a substance increases by 0.63ºC when 565 g of a substance is dissolved in 298K in an organic solvent with a Maʼ 78 density of 0.88 g/cm3, consisting of 5.25 g of C and H. Considering that this solvent is Kf = 5.12 K kg/mol and Kb = 2.53 K kg/mol, and its pure vapor pressure is 103 tor at 298K, find the freezing point drop, vapor pressure and osmotic pressure of the solvent in the solution.
If a 0.580 m aqueous solution freezes at-2.30 °C, what is the van't Hoff factor, i, of the solute? Consult the table of K values.