a. How does manipulating the temperature of the solvent help you determine the suitability for recrystallization? For instance, a good recrystallization solvent should dissolve the solute at (high/low) temperatures and give a high percent recovery of good crystals at (high/low) temperatures.

a. How does manipulating the temperature of the solvent help you determine the suitability for recrystallization? For instance, a good recrystallization solvent should dissolve the solute at (high/low) temperatures and give a high percent recovery of good crystals at (high/low) temperatures.

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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In 6.75g of distillate >130C. After performing all necessary GC calculations, it is determined that this sample is 75.9% isopentyl acetate. What qas the actual mass(g) of isopentyl acetate that was actually in this sample? Answer to 2 decimal places
Q1. Give three criteria for a good recrystallization solvent. Q2. You want to purify 10 grams of benzoic acid that has been contaminated with 0.2 g of salicylic acid. You are given the following data: Solubility in water at 20 °C Solubility at 100 °C (g/10 ml) Compound (g/10 ml) Benzoic Acid 0.029 0.680 Salicylic Acid 0.680 0.029 0.22 6.67 a) What volume of Boiling water is needed to dissolve the 10 g of benzoic acid? (show calculations) b) How much benzoic acid will crystallize after cooling to 20 °C (show calculations) c) Will any salicylic acid crystals form? Why or why not? (show calculations/ reason for answer) d) What is the maximum amount of benzoic acid that could be recovered in the first crop of this recrystallization? (Show calculations) e) How can you prove the purity and identity of the purified Benzoic acid?
A K2SO4 solution is prepared by weighing out a certain amount of the pure solid reagent,dissolving it to 500.0 mL in a volumetric flask. An aliquot was taken from this solution.of 25.00 ml and diluted to 500.0 ml. An aliquot of 5.00 was taken from this new solution anddiluted to 50.00 ml. A chemical analysis of this new solution showed a 0.100%(w/v)in K+. Calculate the weight of the pure solid K2SO4 used for the preparation of the original solution.and its concentration in each volumetric flask. The answer is 2.23x10^2g
The solute in the liquid mixture can be separated from the liquid solvent. O Gas-liquid extraction Solid-liquid extraction Liquid-liquid extraction None of these
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The solvent used in recrystallization could be Question 6 options: a mixture of two liquid; a pure solvent; all options are correct;
6. Calculate the number of moles of magnesium acetate present in 44.8mL of a 9.25 % m/v solution ofmagnesium acetate in water. Use stiochemistry divider lines in between numbers. The answer is 0.0291 mol. 7. A solution is prepared by adding 91.5g of ethanol (C2H6O) to water, making 17L of solution. Calculate theMolarity of the ethanol in this solution. Use stiochemistry divider lines in between numbers. The answer is 0.12M 8) A 0.0880 M Sodium sulfate solution has a volume of 70.0 mL. Calculate the mass of the sodium sulfate inthis solution. Use stiochemistry divider lines in between numbers. The answer is 0.875g
Which of the following solvents is the best to use for recrystallization of Solute A? Hexane Ethyl Acetate Water Diethyl Ether
Connected to DESKTOP-VKHKVG3 A solute added to a solvent raises the boiling point of the solution because Molal Boiling-Point Elevation Constants (Kb) and Freezing-Point nts the temperature to cause boiling must be great enough to boil not only the solvent but also the solute. Disconnect the solute particles raise the solvent's vapor pressure, thus requiring a higher temperature to cause boiling. 06:28 / 31:54 "TRU the solute particles lower the solvent's vapor pressure, thus requiring a higher temperature to cause boiling. the solute increases the volume of the solution, and an increase in volume requires an increase in the temperature to reach the boiling point (derived from PV = nRT]).
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