Answered: How does the data display that water is…

How does the data display that water is a good solvent for recrystallization of benzoic acid? Temperature (C). Solubility(g benzoic acid/L water) 0 1.7 25 3.44 75 21.45 100 56.31

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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Extra information: freezing point depression constant for the solvent (20.0 degrees Celcius kg/mol for cyclohexane)
* 00 LL LI #3 The normal freezing point of a certain liquid X is -2.70 °C, but when 43.3 g of potassium bromide (KBr) are dissolved in 400. g of X the solution freezes at -9.6 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Round your answer to 2 significant digits. °C-kg K. mol Check Save For Later Submit Assignme O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibil MacBook Pro 114 F8 F3 F4 $4 3. 5. 6. P. A G H. K. B alt alt option command command option
Suppose that you have a 1:1 mixture of compounds that is comprised of compound X and compound Y. You desire pure compound X and are planning a recrystallization to enhance the purity. Which solvent below is optimal for your recrystallization? Ethanol (boiling point = 78 °C) Solubility At 0 °C 100 °C Compound X 0.05 g/mL 0.20 g/mL Compound Y 0.02 g/mL 0.40 g/mL Water (boiling point = 100 °C) Solubility At 0 °C 100 °C Compound X 0.02 g/mL 0.05 g/mL Compound Y 0.01 g/mL 0.10 g/mL Methanol (boiling point = 65 °C) Solubility At 0 °C 65 °C Compound X 0.04 g/mL 0.10 g/mL Compound Y 0.02 g/mL 0.30 g/mL Acetone (boiling point = 56 °C) Solubility At 0 °C 56 °C Compound X 0.10 g/mL 0.50 g/mL Compound Y 0.20 g/mL 0.50 g/mL Ethyl Acetate (boiling point = 77 °C) Solubility At 0 °C 77 °C Compound X 0.10 g/mL 0.60 g/mL Compound Y 0.30 g/mL 0.60…
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Be sure to answer all parts. What mass of cesium bromide must be added to 0.500 L of water (d = 1.00 g/mL) to produce a 0.337 m solution? What are the mole fraction and the mass percent of CsBr? g mole fraction mass %
The experimental data in the table was collected during a freezing point depression study where BHT (butylated hydroxytoluene) was the solvent. Mass of BHT Mass of unknown Freezing point of pure BHT Freezing point of BHT and unknown solution Kf for BHT 7.709 g7.709 g 1.252 g1.252 g 74.17 ∘C74.17 ∘C 70.91 ∘C70.91 ∘C 6.83 ∘C/?6.83 ∘C/m Use this data to calculate the molar mass of the unknown solute. molar mass =
Boiling Point Elevation/Freezing Point DepressionT = m KWhere: T = T(solution) - T(pure solvent) * m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb (°C / m) Kf (°C / m) Water H2O 0.512 -1.86 Ethanol CH3CH2OH 1.22 -1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 -5.12 Diethyl ether CH3CH2OCH2CH3 2.02 note that ΔT as defined above will be a negative number for freezing point depression. Therefore, Kf must also be given as a negative number.
Freezing point of pure naphthalene T1 = …....oC Freezing point of solution T2 = ..…..oC Freezing point of depression from graph ΔT = .......oC Weight of naphthalene= 5,028g Weight of Sulfur= 1,011g Kf for naphthalene= 6,8 oC/m 1.Calculate the molality of the solution, m =____________ 2.Calculate the molecular weight of sulfur by using m, W1and W2
show the complete solution and express the final answer with significant figures A. FREEZING POINT DEPRESSION Kf (°C/m) of water 1.86 Freezing Point of Water, °C 0.00 SOLVENT 100.0 g water Mass / Volume added Added reagent Molecular Weight van't Hoff Factor m Freezing Point 20.0 g NaCl 58.44 Answer 1 Answer 2 Answer 3 25.0 g Li2SO4 109.94 Answer 4 Answer 5 Answer 6 10.0 mL 0.150 M ethanol - Answer 7 Answer 8 Answer 9 B. BOILING POINT ELEVATION Kb (°C/m) of water 0.5121 Boiling Point of Water, °C 100.0 SOLVENT 100.0 g water Mass / Volume added Added reagent Molecular Weight van't Hoff Factor m Boiling Point 20.0 g NaCl 58.44 Answer 10 Answer 11 Answer 12 25.0 g Al(NO3)3 213 Answer 13 Answer 14 Answer 15 10.0 mL 0.200 Mglycerol - Answer 16 Answer 17 Answer 18
An aqueous potassium chloride solution is prepared by dissolving 76.8g of KCl in 435.0g of water. What is the freezing point (in°C) of the prepared solution? The freezing point depression constant for water is 1.86°C/m. Freezing point = _____ °C
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