Gravimetric Analysis Unknown 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%.

The purpose of the lab was to determine the percent of water in the hydrate MgSO4 * N2H0 through the process of heating the hydrate, releasing the water molecules, and leaving only the anhydrous magnesium sulfate and also determine the number of water molecules in the hydrate. Throughout the lab, various masses were tooki, including the mass of the evaporating glass with the watch glass, the mass of the evaporating glass, and watch glass with the additional hydrate sample, and the mass of the the evaporating glass, and the watch glass with the dehydrated sample, at two different times, each separated by a five minute interval. After, calculations based on the mass of the left over anhydrous solution were made where the mass of the either the original recorded number for the hydrate was used, or the aftermath dehydrated value of the hydrate. Soon the mass converted

Mole of chlorine : 1.0217g - .221g - .3946 g = .4061 g of chlorine

In experiment A the results from the precipitation of CaC2O4 H2O from the salt mixture were obtained by weighing the items listed on Table 1 on a scale.

The purpose of this experiment was to determine the percent by mass in a hydrated salt, as well as to learn to handle laboratory apparatus without touching it. The hydrated salt, calcium carbonate, was heated with high temperature to release water molecules. Gravimetric analysis was used in this experiment to determine the percent by mass of water in a hydrated salt. The hypothesis of this experiment was accepted on the basis that the percent by mass of volatile water in the hydrated salt would be fewer than 30%. The percent by mass was determined by the mass of water loss devised by the mass of hydrated salt multiplied by total capacity

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.

First students obtained 8 graduated cylinders and labeled them. Each one contained a different ratio of vinegar and water. These graduated cylinders with the liquid were weighed and recorded.Then, students obtained an Alka-Seltzer tablet and recorded its mass. Then one alka-seltzer tablet was dropped into each of the graduated cylinders. Students had to

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

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

1. Label each substance on seven pieces of paper. Put two pieces of magnesium ribbon on the paper labeled “Magnesium”.

The purpose of this experiment was to find the amount and percent of water in a hydrated salt. Hydrated salt contains water molecules chemically bound to it while anhydrous salt is a substance that fire can readily remove the water molecules. Using the gravimetric analysis method, the sample salt was measured, heated, and was measured again after cooled down to room temperature; this procedure allowed the weight of water lost in the salt to be obtained. After two trials, the water in the salt was determined to have an average percent water of -35.04%. The null hypothesis, the heat will not affect the amount of water lost, was rejected ,however, the alternative hypothesis, the heat will allow for there to be water lost, was not supported.

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

When the bag of Unknown substance A was measured, its mass was determined to be 6.49 g, and the amount of moles given was 0.111 mol. Using our experimental method, we determined the molar mass of Sodium chloride was 58.44g/mol. When the mass of Unknown substance A (6.49 g) was divided by the molar mass of Sodium chloride (58.44 g/mol), the answer was 0.111, which was the exact amount of moles given for Unknown substance A. Thus, it was determined that Unknown A was Sodium chloride. The process was repeated and the conclusion of our data is as

The weight of each 50ml beaker (used for weighing the mass of dissolved Potassium chloride after the evaporation of water) should be recorded. If the experimenter were to weigh the mass of one beaker and take it as a default mass, the latter may be a source of error.

One milliliter of 6.00-M phosphoric acid was placed into a 125-mL Erlenmeyer flask using a volumetric pipette. Using a slightly larger pipette, six milliliters of 3.00-M sodium hydroxide was transferred into a 50-mL beaker. Then a disposable pipette was used to slowly mix the sodium hydroxide into the phosphoric acid while the solution was swirled around. Then both the beaker and flask were rinsed with 2-mL of deionized water and set aside. A clean and dry evaporating dish was weighed with watch glass on a scale. Then the solution was poured into the dish and the watch glass was placed on top. The solution was then heated with a Bunsen burner to allow for the water to boil off to reveal a dry white solid. After the dish cooled to room temperature it was once again weighed and the new mass was recorded.