Isolation of caffeine from a tea
To ensure that no water remained in the dichloromethane solution, Calcium Chloride pellets were added. Filter the liquid through a thin layer of cotton into a small test tube.
Be sure to read the MSDS for each chemical and wear safety goggles, a lab coat, gloves, and other appropriate lab attire. Individual spikes on the graph indicate the unique bond energies of certain functional groups.
As a result, large soapy bubbles called emulsions are produced by the polar and nonpolar solutions. Safety Information There are hazards associated with these and any chemicals used in a lab procedure.
Extraction of caffeine from tea lab report discussion
Due to the reaction, pressure built up inside the funnel, requiring the stopcock to be opened to release excess gas following each inversion. You need to separate the caffeine from these compounds. In doing so, the volatile methylene chloride began to evaporate into the surroundings due to the increased room temperature. In effort to prevent another emulsion, a highly saturated solution of salt water was also added to the solutions. As a result, large soapy bubbles called emulsions are produced by the polar and nonpolar solutions. During the extraction phase of this experiment, these bubbles restricted the amount of caffeine released from the separatory funnel resulting in a lesser yield. A 50 mL beaker, along with 2 boiling stones, was weighed in advance with a total mass of Once settled, the solution separated into 2 layers: the polar, brown tea solution on the top and the nonpolar, clear methylene chloride on the bottom. This will cause the caffeine to crystallize out of solution. Carefully remove the liquid using a pipette, leaving the purified caffeine. This spike represents the alkene portion of the caffeine molecule. Place the tea leaves in a ml Erlenmeyer flask. When phenolic acids are reverted back into salts, anionic surfactants are produced4. These pellets are very hydrophilic. To ensure that no water remained in the dichloromethane solution, Calcium Chloride pellets were added.
The second volume of dichloromethane was separated from the water solution and added to the first volume. This will cause the caffeine to crystallize out of solution.
The remaining solution was heated briefly until the volatile solvent evaporated, leaving behind solid caffeine.
By discarding part of the methylene chloride solution, a portion of the caffeine was left behind that affected the overall yield of the product. The spectrometer produced a graph based on measurements of photon energy within a frequency range between and Hz. These pellets are very hydrophilic.
Although the conversion of gallic acid is necessary for the reaction of caffeine and methylene chloride to occur, the phenol anion byproduct of this reaction is responsible for necessary error . When weighed, the beaker, stones, and caffeine rendered a total mass of
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