The followings methods are useful to induce crystallization EXCEPTadding a small crystal of the desired compound, called a seed crystal, to the solutionadding anhydrous potassium carbonate to the solution and cooling it in an ice bathscratching the inner wall of the Erlenmeyer flask with a glass stirring rodreheating the solution to boiling to boil off some of the solvent, and then allow the solution to cool to roomtemperature again to effect crystallization

Crystallization = A purification process. In this process we dissolve an impure solid compound into…

The followings methods are useful to induce crystallization EXCEPT adding a small crystal of the desired compound, called a seed crystal, to the solution O adding anhydrous potassium carbonate to the solution and cooling it in an ice bath O scratching the inner wall of the Erlenmeyer flask with a glass stirring rod O reheating the solution to boiling to boil off some of the solvent, and then allow the solution to cool to room temperature again to effect crystallization

The followings methods are useful to induce crystallization EXCEPT adding a small crystal of the desired compound, called a seed crystal, to the solution O adding anhydrous potassium carbonate to the solution and cooling it in an ice bath O scratching the inner wall of the Erlenmeyer flask with a glass stirring rod O reheating the solution to boiling to boil off some of the solvent, and then allow the solution to cool to room temperature again to effect crystallization

Macroscale and Microscale Organic Experiments

7th Edition

ISBN:9781305577190

Author:Kenneth L. Williamson, Katherine M. Masters

Publisher:Kenneth L. Williamson, Katherine M. Masters

Chapter5: Distillation

Section: Chapter Questions

Problem 7Q: In fractional distillation, liquid can be seen running from the bottom of the distillation column...

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When performing a recrystallization of an impure solid, why is it important to allow the heated solution to cool slowly? Group of answer choices To encourage greater solid solubility. For the molecules of the solid being purified to arrange in organized crystal lattices. To avoid the need for using ice to cool the solution. To trap particles in the crystal lattice.
The question is: A student preforms a crystallization on an impure sample of biphenyl. The sample weighs 0.5g and contains about 5% impurity. Based on his knowledge of solubility, the student decides to use benzene as the solvent. After crystallization, the crystals are dried and the final weight is found to be 0.02g. Assume that all steps in the crystallization are performed correctly, there are no spills, and the student lost very little solid on any glassware or in any of the transfers. Why is the recovery so low? I know it’s becsuse the benzene wasn’t a good choice for the solvent but I can’t explain why. Thank you!
When performing a recrystallization of an impure solid, why is it important to allow the heated solution to cool slowly? Group of answer choices For the molecules of the pure solid to arrange in organized crystal lattices. To encourage solubility. To avoid the need for ice. To trap particles in the crystal lattice.
A 690 g of 59% strontium bromide solution is cooled from 60 oC to a certain temperature. Upon addition of around 2 g of strontium bromide, excess solute above saturation started to crystallize. Total recovered crystals is 146.003 g. How many solute is initially dissolved?
4.0g of potassium hydrogen tartrate was added to 300mL distilled water. The temperature of the solution is 23.1C. The liquid was filtered and 50mL of the filtered solution was transferred to 250mL beaker, two drops of phenolpthalein was added to the 250mL beaker. The concentration of NaOH is 1.0 M that is filled in the 2mL graduate pipette, single drops of NaOH was added to the 250mL beaker until the solution turns pink and the potassium hydrogen tartrate reach the endpoint. The datd of four trials was collected. Please answer the following questions 4) calculate ksp for potassium hydrogen tartrate for each trial and average ksp for thr experiment 5) calculate the percent error in you value of ksp using reference that is found as the theoretical value. 6) why was the temperature of the saturated solution recorded?
4.0g of potassium hydrogen tartrate was added to 300mL distilled water. The temperature of the solution is 23.1C. The liquid was filtered and 50mL of the filtered solution was transferred to 250mL beaker, two drops of phenolpthalein was added to the 250mL beaker. The concentration of NaOH is 1.0 M that is filled in the 2mL graduate pipette, single drops of NaOH was added to the 250mL beaker until the solution turns pink and the potassium hydrogen tartrate reach the endpoint. The datd of four trials was collected. Please answer the following questions 1) calculate the total volume and moles of NaOH required to reach the endpoint for each trial. 2) calculate the molar solubility of potassium hydrogen tartate ( in mol/L) for each trial. 3) calculate the average molar solubility of potassium hydrogen tartate for the four trials. What is the average solubility of potassium hydrogen tartrate in g/L? 4) calculate ksp for potassium hydrogen tartrate for each trial and average ksp for thr…
A salt solution (30% Na2CO3) weighing 1ton iscooled to 20C where the salt crystallizes asdecahydrate. What will be the crystal yield ifthe solubility is 21.5 kg anhydrous Na2CO3/100kg water? (assume that 3% of the totalsolution is lost by evaporation)
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A student performs a crystallization on an impure sample of biphenyl. The sample weighs 0.5 g and contains about 5% impurity. Based on his knowledge of solubility, the student decides to use benzene as the solvent. After crystallization, the crystals are dried and the nal weight is found to be 0.02 g. Assume that all steps in the crystallization are performed correctly, there are no spills, and the student lost very little solid on any glassware or in any of the transfers. Why is the recovery so low?