After purification via extraction, any organic substance should be rigorously dried; otherwise, its further purification via recrystallization will often fail to achieve the desired result. In a typical purification of an organic unknown, a solution of crude product in an organic solvent (i.e. dichloromethane) is what will remain following extraction. Suggest a simple means to remove small quantities of water from this solution.

After purification via extraction, any organic substance should be rigorously dried; otherwise, its further purification via recrystallization will often fail to achieve the desired result. In a typical purification of an organic unknown, a solution of crude product in an organic solvent (i.e. dichloromethane) is what will remain following extraction. Suggest a simple means to remove small quantities of water from this solution.

Macroscale and Microscale Organic Experiments

7th Edition

ISBN:9781305577190

Author:Kenneth L. Williamson, Katherine M. Masters

Publisher:Kenneth L. Williamson, Katherine M. Masters

Chapter7: Extraction

Section: Chapter Questions

Problem 1Q

See similar textbooks

Similar questions

After purification via extraction, any organic substance should be rigorously dried; otherwise, its further purification via recrystallization will often fail to achieve the desired result. In a typical purification of an organic unknown, a solution of crude product in an organic solvent (i.e. diethyl ether) is what will remain following extraction. Suggest a simple means to remove small quantities of water from this solution.
Underline the organic solvent(s) given that would work for the extraction:dichloromethane-water, acetone-water, benzene-water.Concisely explain why the solvent(s) not underlined do(es) not work.
You are employed as a coop student at the Drug and Alcohol Testing Association of Canada (DATAC) developing analytical tests for sports doping agents. You are asked to prepare a procedure for the extraction of methylphenidate, the active compound in Ritalin, from urine samples (consider them as simple aqueous layers, you do not need to consider other components!). The goal of the procedure is to extract the methylphenidate into an organic layer which will then be evaporated, and the residue will be tested for the drug.Your colleague is helping you develop the urine test. They suggest that the urine should be adjusted to a pH above 7 before extracting with the organic solvent. Why is this necessary? Support your explanation with a full arrow-pushing mechanism for the reaction that would occur if the pH was below 7. Include all formal charges, intermediates (if applicable) and products.
You are employed as a coop student at the Drug and Alcohol Testing Association of Canada (DATAC) developing analytical tests for sports doping agents. You are asked to prepare a procedure for the extraction of methylphenidate, the active compound in Ritalin, from urine samples (consider them as simple aqueous layers, you do not need to consider other components!). The goal of the procedure is to extract the methylphenidate into an organic layer which will then be evaporated, and the residue will be tested for the drug.You find that methylphenidate is highly soluble in 2-methyltetrahydrofuran, a bio-renewable solvent. Draw the structure of 2-methyltetrahydrofuran and give two reasons why it is a good solvent choice for liquid-liquid extraction.
The boiling points for the compounds are 118 °C and 35 °C respectively. The solubility for both compounds is the same (8g/100g water). Explain this observation for (i) boiling point disparity; (ii) solubility similarity H-bonds form in diethyl ether; n-butyl alcohol forms H-bonds in water H-bonds form in n-butyl alcohol; diethyl ether forms H-bonds in water H-bonds in n-butyl alcohol; Both compounds form H-bonds in water O Both compounds form H-bonds; Both compounds form H-bonds in water
Under certain conditions, mixing furan with maleic anhydride in diethyl ether yields a crystalline solid with a melting point of 114°C. When melting of this compound takes place; however, one can notice that the melt evolves a gas. If the melt is allowed to solidify, one finds that it no longer melts at 114°C but instead melts at 56°C. Provide an explanation for what is taking place.
What properties should an ideal solvent have to purify an organic compound by recrystallization effectively? (explain extensively) Thanks.
2.1g of sample are dissolved in methylene chloride and the sample is extracted with an aqueous solution of acid and base. Three compounds are isolated - 0.7g of ethyl p-aminobenzoate, 0.6 g of acetanilide, and 0.5 g of benzoic acid. Calculate the % composition of ethyl p-aminobenzoate in the recovered mixture. (Round the answer to 1 significant figure. Give just the number, not a % sign.)
Can you answer and explain this? a. Explain in your own words how the conceptof vapor pressures would differ between simpledistillation and steam distillation and how this appliesto the latter. As we know, steam distillation is used inthe separation of immiscible components, so naturallythere is separation based on affinity towards specificsolvents. Taking the extraction of essential oils as anexample, why would the use of chlorinated organicsolvents such as dichloromethane be useful theirextraction over other organic solvents?
A mixture is made up of low molecular weight carboxylic acid, alcohol and ester. What one step procedure can you use to extract the ester component from the mixture? Describe the process briefly
A student prepares ethyl benzoate by the reaction of benzoic acid with ethanol using a sulfuric acid catalyst. The following compounds are found in the crude reaction mixture: ethyl benzoate (major component), benzoic acid, ethanol, and sulfuric acid. Using a handbook, obtain the solubility properties in water for each of these compounds. Indicate how you would remove benzoic acid, ethanol, and sulfuric acid from ethyl benzoate. At some point in the purication, you should also use an aqueous sodium bicarbonate solution. Outline your procedure using a flowchart.
Naphthalene, C10H8 is insoluble in water but sublimes easily when heated. How could you separate a mixture of naphthalene and NaCl? Suggest two different methods. asap