Essay about Determination of the Composition of Cobalt Oxalate Hydrate

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%.

This experiment is based on determining the chemical formula for a hydrated compound containing copper, chloride, and water molecules in the crystal structure of the solid compound, using law of definite proportion. The general formula of the compound is CuxCly•zH2O, and aim is to determine chemical formula of this compound.

As a group, we obtained our salt mixture of calcium chloride and potassium oxalate, and weighed the mixture. We were able to make an aqueous solution from the mixture and distilled water. We boiled and filtered off the solution, leaving the precipitate. Once the precipitate was dried overnight, it was weighed and the mass was measured. Then we calculated the moles of the precipitate.

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

In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate crystals. There had to be enough hot water in order to dissolve the crystals into the beaker and then add cold distilled water to cool the solution.

The percent of water can be determined in a hydrate by first determining the mass of the hydrate Copper (II) Sulfate penta-hydrate. The substance will be a deep blue color when it is a hydrate. By heating the substance, water is evaporated, removing the water from the hydrate, making it anyhydrous through a simple decomposition reaction. Evaporation is completed when the substance turns from a blue to a white/ grey color. The mass of the water in a hydrate is determined by subtracting the mass of the hydrate from the mass of the anhydrate. The mass of the water is then divided by the mass of the hydrate, and multiplied by one hundred, resulting in the percent of water in the hydrate, which is 36.35%. The percent error is determined by subtracting

The mass percent of water was determined using the mass of water and dividing it by the total mass of the hydrate and then multiplying that answer by 100%. The number of moles of water in a hydrate was determined by taking the mass of the water released and dividing it by the molar mass of water. The number of moles of water and the number of moles of the hydrate was used to calculate the ratio of moles of water to moles of the sample. This ratio was then used to write the new and balanced equation of the dehydration process. The sample was then rehydrated to the original state and the percent of the hydrate recovered was calculated by using the mass of the rehydrated sample by

The purpose of this lab is to determine the percent of water in a hydrate. I learned that copper sulfate hydrate is blue on its own but, when heat is added it will change color to a dim gray. One error that may have occurred is the failure to zero the scale which would ultimately change the math in the equation. Another error that may occur in this lab is forgetting to wait the recommended amount of cooling time, which would change the mass of the elements. At the end if the lab when we look to the questions, it is also beneficial to look at the notes for the lab because it helps with the setup of equations that may come with the questions, also it is very helpful

The goal of this experiment was to determine the empirical formula for a hydrate of magnesium sulfate and water. The technique that was used was measure the mass of the hydrate and then apply heat to evaporate the water. Then determine the mass of water that was in the hydrate and the mass of the remaining magnesium sulfate. The equation for the hydrate is determined by calculating the mole to mole ratio of the water and the anhydrous. The resulting formula will be formated as: MgSO4*_H2O

40 g of ice and approximately 30 ml of sulfuric acid is cautiously added to a 100 mL beaker respectively. Weigh 7.6 g of ammonium chloride and 14.0 g of ammonium bromide and place it in another beaker, crushing the lumps until a powdery mixture remains. The powdery mixture is then transferred to a 125 mL Erlenmeyer flask. Add the ammonium salts into the sulfuric acid mixture. Heat is applied to dissolve the salt. Once the

Dissolve 2.34 g of cobalt chloride hexahydrate (CoCl2.6H2O) in 100 ml of water in an Erlenmeyer flask. While stirring the oxalic acid solution constantly, add the cobalt chloride solution drop by drop. Let the mixture cool in an ice bath. A precipitate will form slowly.

This experiment initially involved the synthesis of an iron (III) oxalate complex with the general

Determine how many grams of Copper Sulfate Pentahydrate you will need for your 100 mL of Water using the solubility curve. (See solubility curve)

Part 3 of the experiment utilized Spectrophotometry to determine the iron content in the iron (III) oxalate complex. The results were combined with findings from Part 1 and

The malachite basic copper carbonate formed as CuCO3 ⋅ Cu(OH)2 shows bright green, whereas that of azurite formed as 2CuCO3 ⋅ Cu(OH)2 shows strong blue. In this study, most of the manufactured copper carbonate was converted to malachite basic copper carbonate of bright green at the reaction mole ratio of >1.20. In the case of low reaction ratio of sodium carbonate, m, the stoichiometric coefficients of CuCO3, is higher than n, the stoichiometric coefficient of Cu(OH)2, so that the amount of CuCO3 is generated is more than that of Cu(OH)2. With increasing reaction mole ratio of sodium carbonate, m is lower than n so that the generation rate of CuCO_3 is lower than that of Cu〖(OH)〗_2. Therefore, copper content increased with increasing sodium carbonate. With assumption of same value of m and n, theoretical copper content becomes 57.5