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%.
The purpose of this lab is to focus on how to make zinc iodide in a different way using compounds instead of elements, which are barium iodide and zinc sulfate. We will see if the reaction between these two compounds will occur and make a prediction by writing a chemical equation. The procedures for this lab are to place a small test tube inside a 50mL beaker and weigh it. Then, using a spatula, add 0.45±0.03 g of zinc sulfate heptahydrate into the small test tube and record the mass. 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.
Experiment 8: Separation of a Mixture of Solids Purpose: The purpose of this lab is to separate the solids mixture containing the iron, sand, benzoic acid and salt. These solids were separated based on the unique properties of different solids such as variation in the magnetic properties and variation is solubility such as ranging from completely insoluble to completely soluble. Procedure: The necessary materials required for this lab procedures was obtained from the labpaq: solids mixture, weighing dish, and digital weighing scale. Each and every solid separated in this lab experiment was weighed using the weighing dish and digital weighing scale. From the solids mixture, the iron filling were separated by using the property of iron fillings that they were attracted towards the magnet.
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
Liquids & Solids Pre Lab Questions: 3pts 1. What are the learning goals of this lab? The goal is to view and experience the melting point and boiling point of different substances. 2. Why is acetamide not allowed in contact with your skin?
One advantage of my proposed procedure about how to separate the sand from the benzoid acid was a strainer which could have stopped sand particles from entering the benzoic acid or to catch any benzoic solid acid crystals from mixing in with the sand. Since the benzoic acid lifted into the top when I boiled the water, it allowed me to pour it right into the paper cup. Also the benzoic acid was popping a lot along the bottom of the beaker during the heating process so I was able to identify the benzoic acid right away. C. Defiantly benzoic acid crystals could have been left behind during the separation process. I noticed some larger crystals of solid benzoic acid rocks left behind
These conditions are more suitable for ionic bonds. That is why the sucrose and salicylic acid did not have good results, because they have covalent bonds. There were a few sources of error that could be improved in the experiment. For example, when the substance was poured into the test tubes, some of the compound remained stuck to the weighing paper. If we used a stick resistant material for this step, the whole 1g would be accounted for.
I also observed that while filtering the benzoic acid-salt mixture that some of the mixture stuck to the sides of the filter and may not have been filtered properly. This may affect the mixture percentages as to that the separate substances may not be as pure as they should be. Calculations -Total Mixture Weight- 6.9 g -Total Mixture Weight based on weight of individual substances- 1.6 g (iron fillings) +1.7 g (sand) + 1.7 g (table salt) + 1.7 g (benzoic acid) = 6.7 g total -Amount of mixture lost during experimentation- 6.9 g – 6.7 g = 0.2 g -Percentage of Mixture- 1.6/ 6.7 = 23.8 % (iron fillings) 1.7/ 6.7 = 25.0% (sand) 1.7/ 6.7 = 25.0% (table salt) 1.7/ 6.7 = 25.0% (benzoic
A graph for the data was also set up with time on the x axis in .5 second intervals and temperature on the y axis. The first task required the freezing point of pure p-xylene be determined. This was done by pipetting approximately 2ml of p-xylene into a polypropylene test tube. The dry thermistor probe was inserted into the p-xylene test tube which was then inserted into an ice water bath. The temperature probe was used to stir the p-xylene and ensured an accurate reading.
The purpose of the laboratory is to determine the number of waters of hydration in aluminum potassium sulfate as well as the purity of the Alum we produce. Experimental1: The procedure for this laboratory was followed closely from Professor Abrams’ lab manual. In Part 1 of this laboratory an aluminum soda can was cut apart and the paint and lacquer was rubbed off with steel wool. Next, the aluminum can was rinsed off with tap H2O and then cut into small pieces. Using the analytical balance 1.0537 g of the aluminum can was weighed out.