When 47.9 g of glycine (C,H;NO,) :are dissolved in 750. g of a certain mystery liquid X, the freezing point of the solution is 3.00 °C less than the freezingpoint of pure X.(Fe(NO.),)Calculate the mass of iron(III) nitratethat must be dissolved in the same mass of X to produce the same depression in freezing point. The van'tHoff factor i = 3.28 for iron(III) nitrate in X.Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.

The colligative property is depression in freezing point, and the formula for depression in freezing…

When 47.9 g of glycine (C,H;NO,) are dissolved in 750. g of a certain mystery liquid X, the freezing point of the solution is 3.00 °C less than the freezing point of pure X. (Fe(NO.),) that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Calculate the mass of iron(III) nitrate Hoff factor i = 3.28 for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.

When 47.9 g of glycine (C,H;NO,) are dissolved in 750. g of a certain mystery liquid X, the freezing point of the solution is 3.00 °C less than the freezing point of pure X. (Fe(NO.),) that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Calculate the mass of iron(III) nitrate Hoff factor i = 3.28 for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.

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

A solution is made by dissolving 0.663 mol0.663 mol of nonelectrolyte solute in 849 g849 g of benzene. Calculate the freezing point, ?f,Tf, and boiling point, ?b,Tb, of the solution. Constants can be found in the table of colligative constants. ?f=Tf= ∘C∘C ?b=Tb= ∘C
Calculate the osmotic pressure of a soln that consists of 43.5g of an enzyme with a molar mass of 9.80*104g/mol dissolved in benzene to make 1.500L of soln at 30.0 degrees Celsius. The density of benzene is 0.879g/mol and the boiling pt constant for benzene is 2.61 degrees Celsius/m. Pure benzene boils at 80.2 degrees Celsius.
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)
O States of Matter Using the Kf and Kb equations with electrolytes 1/5 Donnah The normal freezing point of a certain liquid X is 7.00 °C, but when 67.0 g of benzamide (C,H-NO) are dissolved in 700. g of X the solution freezes at 5.2 °C instead. Use this information to calculate the molal freezing point depression constant Kƒ of X. Be sure your answer is rounded to the correct number of significiant digits. K₁ = 0 °C-kg mol X
The solubility of sucrose near 0°C is 65% by weight. What is the maximum freezing point depression that can be obtained using sucrose? For 100ml of water, how many grams of sodium chloride would create the same freezing point depression?
References Use the References to access important values if needed for this question. The normal boiling point of diethyl ether (CH3CH,OCH,CH3) is 34.50 °C and its Kpp value is 2.02 °C/m. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is testosterone. If 11.37 grams of testosterone, C19H2802 (288.4 g/mol), are dissolved in 286.0 grams of diethyl ether: The molality of the solution is m. The boiling point of the solution is -c. Submit Answer 4. BP/FP Calculations: Solutions of Nonelectrolytes: This is group attempt 1 of 5 Regenerate Group Rack
Calculate the boiling point of solution when 4 g of MgSO 4 (M = 120 g mol¹) was dissolved in 100 g of water, assuming MgSO 4 undergoes complete ionization. (K for water = 0.52 K kg mol−1)
When 4.59 g of a certain molecular compound X are dissolved in 35. g of dibenzyl ether ((C%H,CH,),°). the freezing point of the solution is measured to be 0.9 °C. Calculate the molar mass of X. If you need any additional information on dibenzyl ether, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 1 significant digit. 0 00 0.0 X x10
When 1.38 g of a certain molecular compound X are dissolved in 90.0 g of cyclohexane (C,H,,), the freezing point of the solution is measured to be 6.3 °C. Calculate the molar mass of X. If you need any additional information on cyclohexane, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. x10