After that, dissolve the sample in 2 mL of deionized water and shake the test tube for 1 to 1 ½ minutes to dissolve the solid. Place another dry test tube in a 50mL beaker and weigh it. Find a bottle of barium iodide and record the name and molar mass. Then, weight out either anhydrous barium iodide or barium iodide dehydrate into this test tube and dissolve is it in 2 mL of deionized water. Pour the contents of one of the test tubes into the other and a reaction should occur and you should see a white precipitate of barium sulfate form.
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.
Caloric Content of Food Exercise 1: Determination of Caloric Content of Three Foods Abstract: First I gathered all the equipment needed. Then I zeroed out my balance and measured the mass of the empty beaker. I then put 50mL of water in the beaker and measured the mass again. I put a piece of foil at the bottom of my burner stand and then placed the beaker with water on the beaker stand. I then took the initial temperature of the water.
9/17/2011 Experiment 1: The Mole Concept and the Chemical Formula of a Hydrate Purpose: The purpose of this lab is to learn about the concept of the mole by converting mass measurements, calculating the number of moles in a substance, and calculating the number of moles of water released by a hydrate. With these calculations, one is able to determine the empirical formula of a hydrate from the formula of an anhydrous compound. Procedure: After reading the lab, I went to the store and gathered the materials that were required but not supplied by the lab pack. After I returned, I put on my safety glasses and laid out all the materials that were going to be used in the lab. I realized that the lab did not include 2 aluminum cups used for the experiments so I decided to make them out of aluminum foil.
Once the procedure was performed three times, the collected iron fillings mass was obtained by using the digital weighing scale. After removing the iron fillings, the sand was removed next by using the property of sand that the sand was completely insoluble in the water. The iron free solids mixture was dissolved in 15.00 mille liters of distal water and heated by using stove top in a beaker. The solution was mixed for a while the benzoic acid and salt were allowed to dissolve completely and solubility was enhanced by heating the solution. The solution was decanted into another beaker.
Pour all the filtrate and washings into a 250cm3 volumetric flask. Make up to 250cm3 with 1.0mol dm-3 sulphuric acid(VI) acid. Stopper the flask and invert several times to thoroughly mix the solution. 5. Fill the burette with 0.005mol dm-3 potassium manganate(VII) solution.
The two unknown solids are weighed to a mass of 0.15g each. The unknown solids are dropped carefully into the corresponding Erlenmeyer flask wit 50mL of distilled water. The solid in the water must be dissolved and afterwards add 10 drops of Bromecresol green to indicate the change of color when the solution has been titrated. The flask should start with a blue tint. HCl is carefully dropped into the Erlenmeyer flasks with the primed pipette until the solution turn to a green tint.
The aspirator was turned to medium high, and then the copper was poured onto wetted filter paper. Using distilled water to remove all copper from the beaker. Once completely on filter paper 6mL of acetone was added to the copper to help dry it out. The filter paper was then removed and set down to dry completely. Once dry the filter paper was weighed with the copper on it and subtracted from the original weight to see the amount of copper left after
Materials Protective Glasses | Beaker (250ml) | Stirring rod | Filter funnel | Filter paper | Evaporating basin | Bunsen burner | Heat resistant mat | Tripod | Gauze | Sand | Salt | Matches | | | Method After collecting all the materials needed for the experiment, the students were asked to weigh a mixture of sand and salt (5g) into a 250ml beaker. They also weighed the combined weight of the beaker and salt and sand mixture. They then poured 50ml of distilled water into the beaker, making sure to stir well with a stirring rod to dissolve all of the salt. They then weighed a piece of filter paper, folded it into a cone shape that would fit into the filter funnel, pressing it onto the inner walls of the funnel to make sure no sand would be lost in error. (See diagram below) Water was poured through the filter funnel.
A 125mL Erlenmeyer Flask was used to combine (15mL) of concentrated aqueous ammonia and ammonium chloride (0.0467mol, 2.49g). The mixture was stirred till fully dissolved. Colbalt (II) chloride hexahydrate was ground (6.2g) and added in small amounts to the stirring solution (0.0210mol, 5.2g). As the mixture continued to stir (4mL) of 30% hydrogen peroxide was added drop wise to yield a dark warm slurry. After the effervescence, (15mL) of concentrated HCl was added drop wise to the solution.