RFUMUsing the Kf and Kb equations with electrolytesA certain liquid X has a normal freezing point of 7.50 °C and a freezing point depression constant K-7.03 °C-kg-mol. Calculatethe freezing point of a solution made of 13.8g of glycine (C₂H₂NO₂) dissolved in 450. g of XRound you answer to 3 significant digits.10.3)Calculating and using the van't Hoff factor for electrolytesWhen 132. g of urea (CH₂N₂O)than the freezing point of pure X.are dissolved in 800. g of a certain mystery liquid X, the freezing point of the solution is 7.80 °C lessوCalculate 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= 1.68 for sodium chloride in X.pravidSolutioBe sure your answer has a unit symbol, if necessary, and is rounded to the correct number of significant digits.Mass132.80010.45 =+2.867.800freezionsX-58.44The massThemassfreezing

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Using the Kf and Kb équati -7.03 °C-kg-mol. Calculate хтно A certain liquid X has a normal freezing point of 7.50 °C and a freezing point depression constant K- the freezing point of a solution made of 13.8g of glycine (C₂H₂NO₂) dissolved in 450. g of Xy Round you answer to 3 significant digits. TSIO 2 8: 0.45 + 2.86

Using the Kf and Kb équati -7.03 °C-kg-mol. Calculate хтно A certain liquid X has a normal freezing point of 7.50 °C and a freezing point depression constant K- the freezing point of a solution made of 13.8g of glycine (C₂H₂NO₂) dissolved in 450. g of Xy Round you answer to 3 significant digits. TSIO 2 8: 0.45 + 2.86

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...

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