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Phosphorous And Fluorine Lab Report

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Introduction
Research in chemistry incorporates both microscopic and macroscopic properties. Essential to the properties compounds have both molecularly and environmentally is the ions and metals that make up many compounds. The properties of these chemicals depend heavily on the atoms that make up each particular chemical. Whether the compound is monoatomic, polyatomic, or even a polymer, being able to identify a compound is an essential tool in being able to make predictions and assumptions about the properties a specific chemical may have. Take for example the research being done on phosphorous and fluorine during World War II in Germany and during the Cold War which were able to be used as weapons, or during the early 1930’s when Germany …show more content…

After conducting the solubility test the unknown compound was identified as soluble. This process eliminated calcium carbonate as an option as a chemical. Since the calcium and carbonate ions do not dissociate in water, the solid compounds remains visible; this is not in agreement with the qualitative analysis of dissolved compound. The pH test revealed that the compound was neutral. This eliminated all basic and acidic compounds. Compound not derived from a strong acid and strong base pair, such as sodium acetate, sodium carbonate, ammonium chloride, ammonium sulfate and potassium carbonate, were eliminated as options of the compound. A limitation of this experiment is that if an acid and base were both contaminating the solution a neutral reading may also appear. By using Logger Pro and a pH probe more accurate results for the pH could be taken. The halide, acetate or sulfate test indicated that a halide acetate or sulfate was in the unknown compound. This test is facilitated by the fact that all halide, a few acetate and a few sulfate containing compounds react with silver to form a silver halide, silver acetate or a silver sulfate compound. All compounds not containing a halide, acetate or sulfate (calcium nitrate and potassium nitrate) were eliminated. The sulfate ion test revealed that the compound did not contain a sulfate due to a lack of precipitate formation. This test utilizes the fact that sulfate ions react with barium …show more content…

The rate of reaction between magnesium and hydrochloric acid at room temperature was significantly slow. This process consumed a critical amount of time in lab. In order to synthesize magnesium chloride a sample of 0.254 ±0.001g of magnesium ribbon that was cut into smaller pieces was placed in a solution of hydrochloric acid that was labeled as being 6M. Unfortunately the HCl depleted and excess magnesium remained in solution after a pH test confirmed that all the HCl had been consumed in the reaction. Particles of magnesium were removed from the solution and placed into a 250mL beaker of known mass. The beaker was then weighed and the difference in weight was calculated. This value of magnesium remained was subtracted from the original amount of magnesium to calculate how much magnesium remained in solution. The solution of aqueous magnesium chloride was then heated to evaporate the remaining water and then weighed on a scale. Ultimately the percent error of 41.6% indicates that many sources of error through this process. One major source of error is that magnesium chloride is a hexahydrate, and water moisture from the air may have evaporated into the compound before weighing. Another source of error is that water droplets condensing on the side of the beaker added mass that was assumed to be only the synthesized compound. The two purity tests that were conducted, pH and flame tests, indicated that no basic or acidic compounds were

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Abstract: The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield.

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The compounds tested in included the unknown, Calcium Nitrate, Calcium Chloride, Calcium Carbonate, Sodium Chloride, Potassium Chloride, Magnesium Chloride, and Ammonium Chloride. The next test was the pH test. In this test, the aqueous solutions from the flame tests were used again. A piece of pH paper was dipped into the aqueous solutions, a different piece for each solution. The ensuing coloration of the paper was compared to the pH scale and the

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TLC was used to identify the actual unknown product as well as other products/reactants present in the filtered solution. The procedure was conducted by placing a TLC plate in a developing chamber that is filled with a small amount of solvent. The solvent cannot be too polar because it will cause spotted compounds on the TLC plate to rise up too fast, while a very non-polar solvent will not allow the spots to move. The polarity of the spots also determines how far it moves on the plate; non-polar spots are higher than polar ones. After spots on the TLC form, the Rf values are calculated and used to analyze the similarity of the compounds.

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After flipping it upside-down and placing it into the water, it floated outside of the tube and about half of it came into contact with the outside water. As a result, a bit of the hydrogen gas that formed from the magnesium strip did not make it up the eudiometer; instead, it permeated through the beaker. This logically resulted in a lower value of hydrogen gas volume than if all of the gas made it into the eudiometer. The lower volume of hydrogen gas produced could have skewed our results. In order to prevent this in the future, we suggest securing the magnesium further up the

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So as long as there is enough HCl in the solution to react completely with the magnesium, the results should not change. However, if there is not enough hydrogen with a lower molarity, then the experiment will produce less hydrogen gas since not all the magnesium will be completely reacted. 8. How does Avogadro 's hypothesis relate to the results obtained in this experiment?

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But the difference was no bigger than 0.08, and after the values were rounded the same empirical formula was deduced. So the experiment can be concluded as successful. Evaluation: The method used was simple and easy to follow; however, it did not include how much oxygen was needed to react completely. Also it didn 't mention what magnesium oxide looked like after it finished reacting, so it was a guesswork of determining whether the reaction was finished or not.

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