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
This was done by taking small amounts of the unknown acid. It was then placed into capillary tubes and inserted into the Bibby Sterilin Device. Starting with a high plateau to find a quick melting point and then proceeding to find an actual melting point. The next experiment that aided in finding more characterizations of unknown #2651145-PLF13 was equivalent weight. In order to find the equivalent weight a titration of the unknown acid had to be conducted.
Separation of a Mixture of Solids Purpose To become familiar with separating a mixture of solids, as well as to become familiar with separation techniques dependant on the chemical make-up of a substance. Data Separation Flowchart Initial Mixture (iron fillings, table salt, benzoic acid, sand) | | | | | | | | | | | Put mixture in a cup and hold the magnet over it. | | | | | | | | | Mixture - iron fillings (table salt, benzoic acid, sand) | | | | | | | | | | | Boil mixture to dissolve table salt and hopefully benzoic acid. | | | | | | | | Filter out water with table salt (and hopefully benzoic acid) | | | | | | | | | | | | | | | | | | | | | | | | Mixture - iron fillings and sand (table salt and benzoic acid | | Data Table 1: Experiment Data | | Grams | Percent of mixture | Iron filings | 1.6 | 23.8% | Sand | 1.7 | 25.0% | Table salt | 1.7 | 25.0% | Benzoic acid | 1.7 | 25.0% | Total | 6.7 | 98.8% | Hands-on Labs, Inc Observations I observed that while decanting the sand-table salt-benzoic acid mixture that it appeared that some of the sand may have been decanted out of the beaker as well. 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.
Then weigh the crucible without the hydrate after heating. Record both masses. Next, add CoCl2 ∙6H2O and weigh the crucible. Now place the hydrate and crucible on the hot plate. Observe the color change while it is being heated.
Discussion & Conclusion In this experiment we learned how to synthesize the cyclohexene by dehydration of cyclohexanol. We procedure the first step where we have to mix the components. Then we heat the R.B.F with a fractionating column, distilled water. Then we obtained the layers, and we transferred the organic layer to a small, dry Erlenmeyer flask. We added anhydrous Sodium Sulfate as a drying agent.
This explanation can be demonstrated in table 3 also because the results of the reactions demonstrates that chloride reacted more by the color of the product compared to the color of chloride in the mineral oil. Also it also demonstrates that iodine is the weakest oxidizing agent because the results show that iodide didn’t change much from the color that it showed in the mineral oil. In example 6 we have shown the activity series for the halogens used in this
h) A way to make hard water softer is to put an sodium nitrate and create a precipitate to mellow out the reaction. Another way of making it softer is by removing the calcium ions one way of doing that is by boiling the solution to take out some of the ions. Conclusion: Overall, we determined that sodium carbonate, Na2CO3, is the anion that can be used to precipitate the most metal cations. Also, we learned that the anion sodium chloride, NaCl, could be used to remove silver ions from solutions. The stuff that I found interesting was that how many colours you can get when you mix the cations and anions
An example of use is cleaning compounds of impurities, where different solvents work as a molecular filter that interacts differentially with compound and impurities respectively. In the end of the process, impurities become physically separated from the now pure compound, facilitating further transferring and further repurification / extraction if needed. MATERIALS AND METHODS Acetanilide tert-butyl methyl ether p-tert-butylphenol p-toluic acid 0.5M NaHCO3 3M HCL 0.5M NaOH NaSO4 anhydrous Separatory Funnel Buchner filter paper Sand Bath Microspatula Disposable Pipet heated plate boiling chips support stand Pasteur pipets with latex bulb test tubes (2) utility clamp watch glasses weighing paper melting pint capillary tubes thermometer EXTRACTION •Dissolve acetanilide, p-toluic acid, and p-tert-butylphenol in t-butylmethyl ether •Extract p-toluic acid from the ether layer with NaHCO3 solution •Extract p-tert-butylphenol from the ether layer with NaOH
Micro – scale Reduction of a Ketone to an Alcohol: Benzophenone to Diphenylmethanol with Sodium Borohydride Abstract: Purpose of experiment 2.1 was to perform reduction reaction of benzophenone to diphenylmethanol with sodium borohydride as a reducing agent. The reducing agent was used in excess to ensure complete reduction of the carbonyl group. The product was isolated as a solid by filtration and its purity was checked using Thin Layer Chromatography with different ratios of mixture of polar and non – polar solvents and by checking its melting point, which was 520C - 620C. Infra – Red spectroscopy was not performed, however previously printed graphs were compared and analysed based on tables in Chemistry Laboratory Manual. Purpose of the Experiment: To produce diphenylmethanol from the reduction of benzophenone by using sodium borohydride as a reducing agent.