Preparation of Alum from Aluminum Metal Essay example

My results yielded a high Average Molarity .270M . The ideal would be around 1.000M . Deviation was ± 1.20

Using elemental analysis to determine the percent mass composition of each element in a compound is the first step in creating an empirical formula. There are many different types of elemental analysis, but in this experiment gravitational analysis and Beer’s Law are used. Elemental analysis is first used to find the moles of each element, then converted to mass, and then the percent mass of the element in the product is found (2).

had formed, they were collected by vacuum filtration and weighed. A small amount of the crystals were no weighed due to a lack of toluene with which to rinse the 50 mL Erlenmeyer flask of the last of the crystals.

The empirical formula for silver oxide for trial one is Ag5O4 and for trial two is Ag3O2. For trial one there is 0.451 grams of silver were produced from 0.504 grams of silver oxide. For trial two there is 0.456 grams of silver were produced from 0.500 grams of silver oxide. The difference between the mass of silver oxide and mass of silver is the mass of oxygen that vaporized into the air. There are 0.053 grams of oxygen vaporized into the air for trial one and 0.456 grams’ oxygen for trial two.

Many signs show that a chemical reaction has occurred. Some ways we know there is a chemical reaction are the formation of gas, formation of precipitate, change in temperature, and,or change in color. In part one of the experiment, we know there was a chemical change because of the formation of the white precipitate. We poured the ammonia and water in the flask with alum and water, forming a white, cloudy substance in between the two liquids. The white, cloudy substance between the two is liquids is also known as aluminum hydroxide. The second part of the experiment was very similar to the first, but in the second part we mixed epon salt, water, and ammonia. The precipitate formed from mixing the epson salt, water, and ammonia was called magnesium hydroxide.

3. Examine the luster of the minerals in Figure 1.2 (p. 4 lab book). Place the letter A, B, C, D, or E in

The purpose of this lab was to determine the percent cobalt and oxalate by mass, and with that information, the empirical formula for cobalt oxalate hydrate, using the general formula Coa(C2O4)b.cH2O.

The purpose of this lab is to determine the formula of an unknown hydrate. To achieve this, we heated a hydrate over a Bunsen burner to drive out the water. As a result, the anhydrate is left and the data is used to calculate the mole ratio between the amount of anhydride and water. Then the mole ratios are used to calculate the hydration number, which was 4.8, but was rounded to 5 in the formula. The accepted formula is 〖CuSO〗_4∙5H_2 O and the percent of error was 4%.

The mixture was heated at 120°C using an aluminum block and was stirred gently. After all of the solid dissolved, it was heated for 20 additional minutes to ensure the reaction was complete.

Purpose: To determine the percent magnesium by mass in magnesium oxide and to observe if the percentage composition is constant by comparing class results.

April 2000, the largest gypsum crystal in the world are found in Naica Mexico mine’s Cave of Crystals. Crystals can be made in many different ways. Earth can either make them or they can be made artificially. Crystals can be made out of salt or borax. The earliest crystal grower was Earth. For salt crystal the water starts to evaporate the solution of the amount of salt in the glass that it remains the same. There is not enough water left to keep the sodium and chlorine ions from joining together (What Controls Crystal Growth?). Salt crystals are formed. This experiment will conduct of the type of water will affect the growth of crystals.

In this experiment, a sample of K2S2O8 was prepared by the electrolysis of an aqueous solution of H2SO4 and K2SO4. The peroxodisulfate anion, S2O82-, was also observed for its ability to serve as a counterion for precipitation by preparing a copper (II) complex by reacting hydrated copper (II) sulfate with ammonium peroxodisulfate in the presence of pyridine. This same ability, coupled with its strong oxidizing ability allowed for stabilization of the unusual oxidation state of 2+ for silver which was observed by preparing an analogous silver (II) complex by reacting silver (I) nitrate with ammonium peroxodisulfate in the presence of pyridine. IR spectra for the three products were

Subsequently, two porcelain crucibles were used, weighed, and heated for about 10 minutes and then placed into a desiccator to cool. The two empty porcelain crucibles were first heated because the heat would vaporize any impurities that were originally on the crucible. The first crucible weighed 11.9047 g and the second crucible weighed 12.3735 g. Once the mass of the two crucibles

Minerals are naturally occurring, inorganic, solid, crystalline substances which have a fixed structure and chemical composition. Minerals are an important part of Geology, especially when studying Crystal and mineral growth. Understanding how crystals grow and the difference between slow and fast cooling rates is also important in Geology. Knowing the difference between cooling rates is important because cooling rate changes the texture of rocks and minerals. The purpose for the Crystal Growth experiment is to identify which Solubility and temperature produces larger crystals, and to simulate natural crystal growth. We will achieve the results we desire by conducting the experiment thoroughly and correctly, as well as correctly

An unknown material can be determined by using simple chemical tests and separations which is called as inorganic qualitative analysis. The separation of cations depends on the difference in their propensity to form precipitates. Separation scheme is used to classify cation into five groups on the basis of their physical and chemical behavior opposed to some reagents. Classification is based on whether there is formation of precipitates or not when metal cations react with the reagent. The five groups of cations and the characteristics of these groups are as follows: