Experimental First, we weighed 2 samples, each has 1 gram of NaHCO3-KCl mixture Second, we put the samples in 2 crucibles (A and B) and weighed them. (crucible + sample; WA1 and WB1) Third, we heated both samples on a hot plate for 30 minutes. Fourth, we weighed the samples again (crucible + sample; WA2 and WB2) Lastly, we determined NaHCU3 percentage in the mixture using the following method: WA1 – WA2 x 100% 0.309 WA1 – WA2 x 100% 0.309 * * Results * Theorectically: * Discussion When sodium hydrogen carbonate is heated, new products are formed; sodium carbonate, water vapor, and carbon dioxide gas. This reaction may be presented in a different form with a measure of molecules: @Na2CO3 + H2O + CO2 (solid) (solid) (gas) (gas). Once the reaction of sodium hydrogen carbonate takes place, carbon dioxide gas is released, as well as water vapor.
The major findings were that crude oil has a specific boiling point. And gasoline is the first to be distilled then kerosene and then in the end the lubricating oils. Procedure From the Equipment menu, select Distillation Equipment. Obtain the 100 mL Round Bottom Flask. Now right-click on the flask, and select Heating Mantel from Distillation Equipment then, Right-click on the flask, and select Distillation Head from Distillation Equipment last, Right-click on the flask, and select Condenser from Distillation Equipment.
-Use the titrations of the following chemical reactions: NaHCO3 + HCl (aq) NaCl (aq) + H2O (l) + CO2 (g) 2HCl (aq) + Na2CO3 (s) 2NaCl (aq) + H2O (l) + CO2 (g) Experimental procedure- Two Erlenmeyer flask must be labeled “unknown 1 and unknown 2”. Assure that all containers used are dried and cleaned properly. Two bigger flask are labeled “waste” according to each unknown. A pipette is set up and primed with HCl. The two unknown solids are weighed to a mass of 0.15g each.
The buret had used the NaOH thoroughly rinsed three times because at the first titration the NaOH solution was used. About 50Ml the NaOH solution was in a clean beaker and brought it to experiment area. A funnel was used to fill the NaOH into the buret and recorded the initial volume on the buret to the correct number of significant figures. A pipette was used to take 10.00ml HCl into a clean 50mL Erlenmeyer flask. Three drops of phenolphthalein indicator was added into the HCl solution.
Distillation Experiment CHM226 Background The distillation process is a very important technique used to separate compounds based on their boiling points. A substance will boil only when the vapor pressure of the liquid is equal to the external pressure being applied by the surroundings. Distillations can be used to efficiently purify volatile (i.e. low boiling) compounds. The general concept of distillation involves the boiling of a mixture, resulting in the lower boiling compounds boiling off first.
Gravimetric Determination of Sulfate Purpose The purpose of this lab is to determine the percentage of sulfate in the hydrate by precipitating the sulfate as barium sulfate. Materials Filler paper Sodium sulfate Graduated cylinder Bunsen burner Watch glass Beakers (250 mL, 400 mL) Rubber bulb Graduated pipette Beaker tongs Funnel Filter Paper Sodium Sulfate Drying oven Wash bottle Stirring rod Silver nitrate Hydrochloric acid Distilled water Small test tube Procedures First, .4861 grams of sodium sulfate was placed into a clean 400mL beaker. Exactly 200mL of water and 1mL of HCl was added to the same beaker. A watch glass was placed on the beaker and the solution was heated using the Bunsen burner to a gentle boil. The watch glass was removed with the beaker tongs.
Task 3 To separate a mixture containing water (boiling point 100 0C) butan-1-ol (boiling point 117 0C) I will use fractional distillation. I am choosing fractional distillation as it is the process by which components in a chemical mixture are separated according to their different boiling points . Vapors from a boiling solution are passed along a column. The temperature of the column gradually decreases along its length. Components with a higher boiling points condense on the column and return to the solution ; components with a lower boiling points pass through the column and are collected.
Procedure: Mix the two solutions together. Stir by stir bar and stir plate, swirl the mixture in the flask by hand, or mix by transferring the mixture back and forth between the two flasks. Stir until the colorless solution turns blue (about 10 seconds). Clean-Up: Remaining blue solution can be washed down drain with water . Background: For the entire explanation of this demo see Shakhashiri's Chemical Demonstrations, Vol.
For a single extraction, use a 50mL graduated cylinder and measure out 50mL of the benzoic acid solution into a 125mL separatory funnel. Add 10mL of methylene chloride (dichloromethane or CH2Cl2 for abbreviation which is the organic layer), the extracting solvent, to the funnel. Shake the funnel for thirty seconds pointing it away from the student and self. Release gas buildup by opening the stopcock of the separatory funnel. This is called the shaking and venting procedure.
Before the experiment, take out the fridge water and measure out three cups and pour it into the one quart pot and measure the water temperature before placing it on the stove. Then turn the stove on to maximum heat as well as the timer. While the water is reaching to the boiling point measure and note the temperature for every minute. Next, let the stove and the pot cool down for few hours. Then take jug with room temperature water and pour out three cups into the pot.