The primary of this lab is about the hydrate. The hydrate is a compound formed by an ionic bond combined with the water molecule (known as “water of hydration”) attached to it. So for every formula unit, there would be some amount of water molecule combined with the ionic compound and would act as a single compound. Our theoretical hydrate for this lab was CuSO4 * 5H2O. To remove the water from the compound and get the mass of the ionic compound, you need to follow the dehydrating procedure by heating. That would separate the ionic bond (CuSO4) from the water molecule (5H2O) once it reaches certain decomposition temperature. And to physically determine whether or not the water of hydration is removed, see the color, in our case, turning white from blue. Once the water molecules have entirely evaporated, the mass left would be the weight of the ionic compound (mass of CuSO4 in grams). …show more content…
The empirical formula is a similar molecular formula but in its simplified ratio. While calculating, you need to find the percent of a part of the compound from the whole compound. Then find the moles of each composition and then calculate mole to mole ratio between copper(II) sulfate and water to achieve the possible empirical formula. But for the mole to mole ratio to work, you need to know the law of definite proportions. It says that every chemical compound would have certain proportion, by mass, of its composition and that ratio cannot be changed. So for example a mole of water would always have 1 mole of Oxygen and 2 moles of
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%.
Empirical formulas represent the ratio of atoms in a formula. It is expressed in the simplest, small, whole number ratio. The molecular formula can either be the empirical formula, or a multiple of the empirical
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.
The percent by mass of volatile water was determined by the measurements from the hydrated salt and the mass of the water loss.
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 mass of the water was found by subtracting the original mass of the hydrate by the anhydride, that was found after heating the hydrate and evaporating the water. However, if the hydrate was not fully heating and there was still excess water remaining, this excess water mass would be included in the anhydride mass. This would make the mass of the anhydride larger and the mass of the water smaller. If the mass of the water was smaller, then the amount of moles of water would also be smaller. The mole ratio of anhydride to water would be larger because the denominator in the ratio, water in this case, would be smaller, so the entire ratio would essentially increase. This would mean that the number of molecules of water would be smaller as a result.
The Empirical Formula is a formula that shows elements in a compound. The molecular formula gives the amount of atoms that each element has in a compound. These formulas were used to calculate and find elements that were given prior to the crash. The formulas also helped our team find out which passengers had each of the possible materials on the flight.
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
Then 8.0g of copper sulfate crystals were placed inside the beaker and the mass was recorded for the actual crystals. 50 mL of water was added to the beaker with the crystals. The ring stand was set up with the wire mesh on it and one partner should place the mixture in the beaker on it should be heated without letting the mixture boil. Stir the mixture and heat until the crystals are dissolved. While one partner does this, the other should obtain 1.5g of iron filings in a measuring cup and records the mass. Then the iron filings should be added small amounts at a time to the heated solution. Stir continuously until all the mixture is added to the beaker. Then it sat for 10 minutes and observations were recorded. Record the mass of a filter paper and set up a filtration apparatus with the filter paper in a funnel over an Erlenmeyer flask. Decant the liquid through the paper slowly trying not to allow any solid to get on the filter paper. Then with de-ionized water, rinse your solid in the beaker and let the solid settle then decant the liquid. Repeat the washing twice more and in the last time guide all the solid into the filter paper. Then place the filter paper on a watch glass and then into a warm oven to dry. After it is cool, record the mass of the watch glass, filter paper and solid. If there is not enough time to cool, you may have to do it the next
There is a very easy way to find the empirical formula of a compound using the mass percentages found through elemental analysis. First, convert the mass percentages to a mass, assuming that the compound is 100g. Then convert each mass into moles using the molar masses. Then divide each of these moles by the element with the smallest amount of moles. That is the ratio of the empirical formula. Just make sure that the numbers are in whole numbers, if not, multiply by common denominators to get all of them to a whole number (3).
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 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
The powdered cobalt oxalate hydrate was weighed to about 0.3 g and placed in a pre-weighed crucible. The crucible and the cobalt oxalate were then heated until the cobalt oxalate decomposed into a stable, black solid, or Co3O4. Once the crucible was sufficiently
3) Repeat the drying process just to be sure that the copper is completely dry, and again determine the mass of the copper and the beaker.