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.
In your right hand hold the pipette with Na2S203 and squeeze the Na2S203 into well #1 and start timing with your stopwatch. 16. Observe well #1 while a reaction occurs. Stop your watch when you can no longer see the X sign through the bottom of the well. Record the exact time in seconds under the Trial 1 column in the Data Table
Obtain an Erlenmeyer flask that has a vacuum opening and attach the vacuum tube to it 8. Insert funnel and rinse the funnel with distilled water 9. Turn vacuum on and pour the pink solution into the Erlenmeyer flask, the precipitate should stay on top of the filter 10. Rinse the beaker out until all residue is gone 11. Try to rinse the precipitate in the funnel until the pink color is gone 12.
Using a measuring cylinder, add 50cm3 of 1.0mol dm-3 sulphuric(VI) acid to the thyme extract in the conical flask. 8. Titrate the solution in the conical flask with the potassium manganate(VII) solution until a pale pink colour persists for 10 seconds. 9. Repeat the titration until there are two titres within 0.1cm3 of each other.
That told me it was the end point of the titration. When I added the base to the acid, I noticed that the indicator in the acid turned pink after reaching the end of the titration. Procedure Part 1: *First I had to measure the pH of 0.1 M hydrochloric acid. Get a 100 mL beaker from the equipment menu Right click on the beaker, select chemicals, and add 50 mL of 0.1 M hydrochloric acid. Measure the solution by right clicking on the beaker and choose pH meter *Then I had to measure the pH of 0.1 M sodium hydroxide Get a 100 mL beaker from the equipment menu Right click on the beaker, select chemicals, and add 50 mL of 0.1 M sodium hydroxide.
We used .112 moles of bromobenzene, and .0103mole of magnesium moles of Methyl benzoate was the limiting reagent in the experiment. In calculating the theoretical yields. We used the limiting reagent multiplied by the molecular weight of the product. The initiation of the Grignard reaction began after about ten minutes of gentle heating was applied to thereaction flask containing the crushed magnesium turnings and first portion of the bromobenzene/anhydrous diethyl ether solution. This initiation was evident by cloudiness and graying of solution as well as the evolution of bubbles off the surface of the metal.
Riya Singh Banita Sathpathy Period 1 Analysis of a Commercial Bleach Purpose The purpose of this experiment is to determine the amount of sodium hypochlorite in commercial bleach by reacting the bleach with sodium thiosulfate. Procedure In this experiment a solution of sodium thiosulfate of known concentration will be added to the bleach using a buret in a titration procedure. The disappearance of the dark blue color of the starch- iodine complex will signal the end point. Data Trial 1 Trial 2 Trial 3 Initial Reading (ml) 0 0 0 Final Reading (ml) 35.7 36.0 36.6 Volume of Na2S2O3 35.7 ml 36.0 ml 36.6 ml Calculations and Analysis 2 S2O3-2 = I3- = I2 = ClO- Therefore looking at the equation above, we can conclude that for every mole of sodium thiosulfate we need half a mole of sodium hypochlorite. (35.7+36+36.6)/3=36.1 ml is the average volume of the Na2S2O3.
Observing Changes – Materials & Procedures Materials Water Copper (II) sulphate (Powder) Copper (II) sulphate solution Iron nail Sodium carbonate Hydrochloric acid Magnesium ribbon Flame (candle) Sugar Aluminum foil Test tubes Test tube rack Tongs Medicine dropper Spoons Beakers Safety goggles Scoopulas Procedures Water and Copper (II) Sulphate Procedure 1. Add a small amount of solid copper (II) sulphate to a test tube with a scoopula. Record the physical properties. 2. Write a hypothesis on what you think will happen when water is added.
Add the HCl SLOWLY to the magnesium by running it down the side of the beaker. Adding the acid too quickly will result in the spattering of the acid. Write down any observations of the reaction. 6. After all the acid has been completely added and the reaction has stopped, use a pipette to add a few extra drops of acid into the beaker until the reaction stops.
Obtain a clean-dry test tube. Place 0.3g of the unknown substance in the test tube. Next, add 10mL of distilled water to the test tube. Mix with a stirring rod until unknown is dissolved. 2.