Distillation and Chromatography

Objectives Separate the components of a solution using distillation and chromatography Determine physical or chemical properties which proves separation was successful Determine Vapor Temperature variations during the distillation.

An Introduction to Separations

What is Separation The division of chemical mixtures into its chemical components by physical means. A single substance that has no other substances mixing with it is called a PURE SUBSTANCE. If there is something else mixed with it, it is a mixture.

Why Separations Most Chemicals are natural products that must be separated into pure chemicals for use in industry or research.

How to Separate Separations are achieved through mostly physical means. All chemicals have different physical characteristics. The differences in the physical properties are exploited to separated different molecules.

Example Physical Properties Boiling point Melting point Charge state Partition Coefficient Vapor Pressure Solubility

Physical Properties of C2 Molecules

Types of Separations Re-crystallization Selective Precipitation Solvent extraction Electrophoresis Distillation Chromatography Field Flow Fractions Super Critical Fluid Hyphenated methods

Introduction to Chromatography

The Master British biochemist Richard Synge won the 1952 Nobel Prize in chemistry. He developed partition chromatography, a technique for identifying and quantifying the component parts of such substances as proteins, carbohydrates, and nucleic acids.

Elements necessary for Chromatography Mobile Phase Stationary Phase Sample inlet Detection

Types of Chromatography

Types Of Adsorption Packings Paper Cellulose Starch Sugars Magnesium Silicate Calcium Sulfate Silicic Acid Silica Gel Florisil Magnesium Oxide Aluminum Oxide Activated charcoal ODS Synthetic packing

Thin Layer Chromatography

Developing Chromatograph

Liquid Column Chromatography

The Packed Column

High Pressure Liquid Chromatography

Distillation is… The separation and purification of a mixture of components based on the different volatilities of each component. The volatile components are vaporized, then condensed, and collected.

What is in our mixture? 1)Water 2)Ethanol 3)Red Dye 4)Blue Dye

Volatility Water is less volatile than ethanol because water’s intermolecular forces are stronger than those of ethanol.

Phase Equilibrium Temp %Ethanol %Water º vapor liquid 83% 17% 67% 33%

Modifications to Procedure 1 ml direct pipette with pump Small plastic beaker for density determination Dye Mixture Plastic graduated dropper for food dye Ice Large beaker for Ice Bath Chromatography Kit 4 vials for each component isolated

Procedure modifications Prepare a solution containing 25 % V/V Ethanol Water Solution Volume of solution prepared should not exceed 25 % of volume of pot Flask Determine Volume by the following Equation Volume of Pot Flask *.25 = Total Volume of solution prepared Using a Pipette and Balance determine the density of the solution prepared

Chromatography Analysis Wet the column using eluent which is designated as the most polar Place the.5 ml of solution prepared into reservoir of Column Chromatography apparatus as demonstrated by Instructor Draw into column the solution Add the polar eluent into the column until one of the dyes can be isolated into the small vial provided

Chromatography continued Place the less polar eluent into the reservoir above the column. Draw the eluent into the column as instructed. Isolate the second dye and place into labeled vial

Distillation Using Logger pro determine the temperature which is most constant during the distillation. Do not allow the vapor temperature to exceed 90 degrees Celsius Test the combustibility of the solution prepared and the combustibility of the components isolated Determine the density of the original solution and density of the separated components.

Questions Answer all questions in lab Using the most constant temperature reading obtained during the distillation determine the % alcohol in the Vapor. Which of the Dyes is more Polar and Attracted to the more polar Eluent