C. The sand recovery percentage being higher than the original sand percentage could take place if all the iron was not removed from the mixture. D. If the sand was not dry when it was weighted, if the Benzoic acid was not filtered properly. These could have increased the percent of error. Conclusion: I thought it was neat to see how each solid separated from the others. The magnet collecting the iron caught everyone’s attention.
You can go to the web for flow chart examples. Flow Chart: (3 pts) Based on the physical properties (solubility, density, melting point, etc.) of sand, NaCl (table salt), benzoic acid, and iron filings, prepare a flow chart for the experimental procedure for this experiment and include it in your report in the table on page 2. Then you will be ready to follow the experimental procedures as described in the lab manual. If you make any changes to the experimental procedures, please record these changes below: Flowchart: (complete before
One student did not stir the mixture before decanting the water a. This error could cause the percent of sand calculated to be too high. When the mixture is stirred it allows for the sand and salt to separate away from each other enough for the salt to be dissolved and the sand to sink to the bottom. If it is not stirred correctly the salt may not fully dissolve leaving it mixed with the weight of the sand you are using to calculate the percent. b.
Procedure: Weigh out the mixture, and then use different techniques to separate them from each other. Using the magnet to separate out iron filings, boiling the substance to separate out the sand, and filtration paper to separate the salt and benzoic acid. Once substances are separated and dried, weigh them out to receive a total amount. III. Experimental Data: The original weight of the mixture before separation was 4.6g.
Results: Please see attached the final results and questions to go with Lab #3. Discussion: I realized that as I was going through the different steps of taking out the solids, I seemed to be losing some material, whether it be from spilling some here and there or from factors that I could not help, like the sand getting stuck to the side of the glass. However, my percent of mixture total came close to 100% meaning that my solids may not have been as exact as when they first started in the bag, but they were close enough to gain data from. Report: Data Table 1: Experiment Table Grams Percent of Mixture Iron Filings 1.5 23.8% Sand 1.7 26.9% Table Salt 1.5 23.8% Benzoic Acid 1.6 25.4% Total 6.3 99.9% In order to get these results shown in the graph I used a formula which took a specific
Ailsa Cottam 28.10.13 Separating salt and sand. Introduction In this experiment students were asked to separate a mixture of salt and sand, illustrating the fundamental means of separating a mixture of an insoluble material from one which is soluble. Aims/Hypothesis Students were asked to perform an experiment into the separation of a mixture of salt and sand, identifying the calculations of both sand and salt once going through the separation process. The separation techniques that were used in the lab were Evaporation and Filtration. 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.
Since a dispersant is able to break down and separate oil from other areas it will be able to get the oil out into the open or to any area you would choose to contain it. Dispersants similar to dish soap will be very beneficial. The use of skimmers would follow after the dispersants have taken affect. Objects similar to long cardboard that would be able to move the oil into a large bubble without actually making the oil disperse out should be use. Once as much oil is contained into a large blob in one area the next best step is to block it off and prevent it from being able to leave.
5. The burette was then refilled with the NaOH and the meniscus was adjusted so that it sat at 0.0mL 6. The pipette was filled with the acetic acid and then drained once again to ensure the pipette wasn’t contaminated as otherwise the obtained results could have been incorrect. 7. The pipette was then filled with 25.0mL’s of acetic acid and then drained into a conical flask, to speed up the process both of the conical flasks were filled with 25.0mL of the acetic acid.
LIQUID-LIQUID EXTRACTION OF BENZOIC ACID J Wright Organic Chem Lab 1 Tuesday 1:40-5 Ian Stubbs LIQUID-LIQUID EXTRACTION OF BENZOIC ACID PURPOSE: The purpose of this experiment was to extract benzoic acid from an aqueous of benzoic acid using methylene chloride, use liquid-liquid extraction to calculate the distribution coefficient of benzoic acid and to determine whether a single extraction or multiple extractions are more efficient. Add in the table of physical constants. See the attachment for the lab format. PROCEDURE: Gather a two stock solution that includes; 0.02M of sodium hydroxide (NaOH) aqueous solution and 0.02M of benzoic acid aqueous solution. For a single extraction, use a 50mL graduated cylinder and measure out 50mL of the benzoic acid solution into a 125mL separatory funnel.
The dry sands would absorb the moisture out of the bodies. Without moisture, bacteria on the bodies couldn’t cause decay. Egyptians discovered that the bodies naturally mummified when scavenging jackals began digging up the mummified bodies for food (“All about Mummies”). It was decided that the dead needed a more proper way of burial They started to improve the burial placed by piling rocks on top of the body to keep the jackals from digging up the bodies. They also began lined the pits with straw or animal skins.