The Formula And Percent Water Of Hydrated Magnesium Sulfate

The purpose of this experiment was to determine the formula of a hydrate CuSO4 specifically, determine the amount of water in that hydrate. In order to do so, a sample of the hydrate was placed in a crucible that sat above a flame. The flame, provided by a Bunsen burner, aided in the evaporation of the water existing in the hydrate. By recording the mass of the hydrate sample before and after it was heated, the water lost due to evaporation could be calculated; 5 molecules of H2O was concluded. This information allowed the formula of the hydrate to be determined: CuSO4 • 5H2O(s)

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 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 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.

In Rosemary Jolly's class, students performed the hot plate procedure in order to evaporate the water from the unknown hydrate.  The equipment that the students used were two 100-mL beakers, an analytical balance, a hot plate, and a clean glass rod to stir the substance.  Students obtained about 1 or 2 g of the unknown hydrate into one of their 100-mL beakers.  They determined the combined mass of the sample and the beaker.  After doing this, they placed the beaker onto a hot plate that was on a medium setting.  Using the glass rod, students stirred their beakers in order for all of the unknown hydrate to melt until a dry powder appeared.  Once the dry powder appeared in the beakers, the students took their beakers off of the hot plate in order to cool to room temperature.  They placed the beakers on an analytical balance to record the mass of the beaker and residue.  This information was used later in the experiment to find the number of moles of water per formula weight unit of magnesium sulfate.  Students repeated the procedure with their second 100-mL beaker.  Once the second trial was completed, they used their data to determine the average number of moles of water present in the magnesium sulfate

The purpose of this experiment is to determine the empirical formula also known as the simple formula of a compund known as a hydrate.

Introductory Paragraph- In this lab, we tested how much water was in a 3.00 gram amount of hydrated MgSO4 (Magnesium sulphate). MgSO4 is a salt; salts are often associated with water being in their structure. This lab was conducted so that we would be able to find the formula for the amount of water in the sample of magnesium sulphate. The goal was find the formula of a hydrous substance if you are given two masses.

6. Allow the crucible to cool to room temperature. Then weigh and record the mass of the crucible, lid, plus the residue that remains. Note that the weight of your sample is expected to decrease by at least 30 % of its original mass (~ 0.3 g).

7. Sealed the first test tube of 0.2 g of baking soda with a rubber stopper and inserted the other end of the rubber tubing into the spigot placed in one hole rubber stoppers. 8. Set up retort stand #1 and attached the test tube at an angle of 45o using utility clamp #1. 9.

“The simplest empirical formula of a hydrate is salt.xH20(S) --- Anhydrous salt + xH20. When heating the hydrate find the mass loss using w1 - w2. W1 and W2 are the masses of the hydrate and anhydrous salt. Perform the necessary calculations to find the moles of water and the moles of the anhydrous salt, using the molar mass of the anhydrous salt.

Turned on the Bunsen burner to 80oC, placed underneath the angled test tube with sodium bicarbonate, and using a functional flint lighter, carefully held it slightly off center of the barrel of the burner and a few inches above from the top, and lit the Bunsen burner

The purpose of this experiment is to determine the mass of a piece of the magnesium, without weighing the magnesium on a balance. To determine the mass of the magnesium, without weighing is to use stoichiometry of a chemical reaction to be able to determine the mass of the magnesium. If the volume of hydrogen gas produced can be determined by using the combined gas law equation, then the mass of magnesium being used can be determined using

This lab demonstrated both the law of definite proportions and the law of conservation of mass. Because hydrates are compounds with a a constant composition and because the waters of hydration(water molecules bound to the salt crystals) can be relatively easily driven off by heating, the amount of water present in the hydrate can be

First you will need to light your burner to the hottest part of the flame before starting your gram stain. After the burner is lit you will move to

The process of hydrate nucleation both in natural and in techno genic conditions has a common basis when hydrates form from free water and gas. However, additional conditions which are determined by capillary pressure, surface tension, salt content of the fluid and capacitative properties of medium are applied during hydrate formation in a porous media. The formation of gas hydrate has to be categorised fewer than two groups 1) formation of hydrates from dissolved gas when the rate of hydrate accumulation is determined by the diffusive influx of gas from adjacent water and 2 from free gas contained in pores gas or gas condensate deposit transforms into gas hydrate one during a change in thermodynamic conditions. For the first case the molecules