Formula Of A Hydrate Lab

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%.

I. LIQUID - Identification of an Unknown Liquid: Using the physical properties of Solubility, Density, and Boiling Point.

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.

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.

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

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 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

Our purpose in this lab was to create four solutions of the same components and different concentration. I found the concentration in Molarity (mol/liter). I would dilute a solution to create new solutions, using the formula M1xV1=M2xV2 where M=molarity and V=volume. In this lab, there were four solutions, Solution A, Solution B, Solution C, and Solution D. The solute or substance that dissolves was sugar and the solvent or substance that the solute dissolves in was water. For Solution A, I weighed 3.42 g sugar and diluted to 100 mL to get a concentration of 0.10 M and the color of bright red. For Solution B, I weighed 0.342 g sugar and diluted to 100 mL to get a concentration of 0.010 M and the color of pink. For Solution C, I measured 10

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

Before we entered the lab, our instructor shaved the magnesium in to small pieces. The magnesium was measured out to fill about the bottom curve

The lines in Figures 6 (A) to 6 (F) indicate predicted values, using fitted rate constants for the reaction. The rate constant valueswere found to increase as expected as the temperature was increased. The activation energies were determined from the temperature dependency of the rate constants to be 831, 2494, 3076 and 2660 J/molfor hydrazone, tryptophol, cinnoline derivative, and polyindole formation, respectively(Table 2). The values indicate the amount of energy required to cross the energy barrier so that,the reaction can takes place. The activation energy for hydrazone formation is low(Table 2) indicating that, the reaction takes place at lower temperatures buttheactivation energy barrier is higherfor tryptophol formation.

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.

The second procedure called for us to heat a number of other hydrates and test their vapors for any evidence of acid just as we had done in the previous experimental procedure. The results for the heating of each individual hydrate posed a different conclusion