Separation Of Myristic Acid Lab Report

The purpose of this experiment is to isolate myristic acid from the triglyceride, trimyristin, by using basic hydrolysis followed by acidification. First, tert-butyl methyl ether is utilized to extract the trimyristin and recrystallize from acetone to yield pure trimyristin. Sodium hydroxide, water, and ethanol are utilized to convert trimyristin to glycerol and sodium myristate. Finally, hydrogen chloride and water are applied to convert sodium myristate to myristic acid via hydrolysis. This experiment illustrates the paramount process of obtaining a pure organic yet medical compound from a natural source.

Reaction Scheme: Table of Reagents:

Compound MW (g/mol) BP (℃) MP (℃) Density (g/mL)

Trimyristin 723.16 311 56-57 0.85

NaOH 40.00 1388 318 2.13

Water (H2O) 18.02 100 0.00 1.00

HCl 36.46 -85.05 X 1.49

EtOH 46.07 78.29 0 0.79

Table of Products and Byproducts:

Compound

Trimyristin was then processed to produce glycerol and sodium myristate using sodium hydroxide, ethanol, and water as reagents. After, hydrogen chloride and water were applied to convert sodium myristate to myristic acid via hydrolysis. In terms of reagents and product’s character, sodium myristate has the yellowish look in polar solutions like water because it is lipids that congregate into small droplet called a micelle. Thus, the nonpolar sides congregate on the inside of the micelle and polar ionic ends at the outside surface of the globule. The nonpolar inside dissolves the grease molecules and the ionic outside is washed away. As the result, the myristic acid will form.

Based on the stoichiometry of the reaction, one mole of trimyristin yields three moles of sodium myristates, therefore three moles of myristic acids are produced. In this experiment, 0.062 grams of trimyristin produced 0.05 grams of myristic acid. The percent yield is 84.75%. The 100% theoretical yield should be 0.059 grams of myristic