When our filtered solution started to cool off over time crystals started to form. Then we used the vacuum filtration system to separate the crystals from the cold water we used to wash them. After letting our crystals dry over night in a sealed beaker we weighed them the next day to find out what percent of crystals we were able to recover. After weighing the crystals I determined we were able to recover 4.8 grams of the original 6 grams of Acetanilide for a recovery rate of 80%. Part Two: 1: The purpose of this experiment was to remove the contaminants from the impure Acetanilide and see how much of the crystals we could recover through the recrystallization process.
The reflux apparatus was place in the aluminum block. The block had been heated around 15 minutes which was to 120-130°C As the mixture was warmed, the white solid that formed was dissolved. The apparatus was lifted out of the aluminum block after a period of heating. Also, the flask was placed under the tap water to cool down the mixture to room temperature. Carefully 0.5mL increments of 3M sulfuric acid was
The solution with the precipitate was divided in to two tubes and centrifuged. The formed precipitate was left behind after washing the liquid out. Then we added another 5 mL and centrifuged again and washed the tube again. Eventually when got our Zinc Hydroxide in the test tubes. We then performed the two tests: Acid and base.
We selected a spirit burner and recorded the name of the fuel into our table; we also included the mass of the whole burner. We then clamped the steel can so that the spirit burner will fit under it. We light the wick of the spirit burner and placed it underneath the can. After we used the thermometer and to gently stir the water when the temperature increased by 20 we put the lid on the burner to put the flame out, we then recorded the new mass of the whole burner including the lid and fuel inside. We repeated thus experiment twice with each fuel, using clean water each time.
We rinsed a pipette with some of the sample, filled curettes between 2/3 and 3/4 full with the samples, put a curette in the cell holder and make absorbance measurements. If we see the absorbance of the sample run out off the computer screen. That means it is too concentrated so we need to get some dilution of the sample. To dilute it, we took 1mL of the stock reference sample and dilute with water until the intensity is less than the stock reference sample. Measure the new sample volume.
Graduated cylinder 8. Calculator 9. Wash bottle Procedure: To commence, first I gathered all the material needed to keep from being too messy with the experiment. Next I went to collect my unknown liquid and metal since the material and purpose was to find the mass and volume of them and located their place of origin from the data collected. Once all the equipment has be gather, step one was to clean the flask because a dirty flask might have an effect on the precise mass of it.
Allow the crystals to dry for 1 week then, weigh it, take a MP, and calculate the % yield. * Assemble the apparatus for reflux using the diagram (see figure 1), place boiling chips or a stirring bar in the bottom of the flask. * Weigh 2grams of finely ground nutmeg and combine with 10ml of diethyl ether in a 50ml round bottom flask. * Place a heating mantle under the round bottom, turned on and the heat was slowly adjusted until the mixture starts to boil for 45minutes, then let cool to room temperature by sitting it on the lab bench. * Pour a little ether over the nutmeg residue on the filter paper so that any Diethyl ethanol traces clinging to it is washed down and mixed with the filtered liquid underneath.
Flame Tests – Identifying cations Abstract: My objective of this experiment is to identify cations present in water samples. To do this I will be doing 7 experiments using different types of metal ions. To do this I will clan the flame test wire by dipping it into acid, then heat nichrome wire in a Bunsen flame until no colour is visible in the flame. Then dip the wire into acid, then into salt solutions and hold wire in edge of flame and finally note the colour of the flame, then repeating this for all the salt solutions. Introduction: This report is based upon my hypothesis taken out in an experiment.
Lab Report: Crystallization of phthalic acid from water (microscale) Abstract The 0.60 g of phthalic acid is put in a water solution, which is brought to a boil to dissolve the acid into water. After the solution was clear with just the rock visible the test tube solution is now cooled in ice and stirred till crystals appear. Excess water is then removed, then the adding of ethanol is done to separate the water from the crystals. Tube is then placed in a beaker of hot water which aids in the removal of the solvent. After drying the compound the percent recovery was found to be 70%.
I then measured hot tap water versus boiling water, and then cold tap water versus water with ice, and recorded the temperature that was read on the thermometer, and then converted the temperature from Celsius (C), to Fahrenheit (F), and Kelvin (K). To understand how to measure mass, the lab required the following material: pen or pencil, 5 pennies, 3 quarters, 4 dimes and a key. Then I used the digital scale to measure the following objects to obtain its mass and recorded the data. For exercise 2, volume, density and concentration, I started off measuring the graduated cylinder to get its mass. From that mass, I was