Lab Report Hydrated Magnesium Sulfate

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 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

Place the beaker on the hot plate, place the thermometer in the beaker and set the hot plate to 5oC.

Introduction: The purpose of this lab will be to determine the percent water in an unknown hydrate, determine the moles of water present in each mole of the unknown substance, and to use the molecular mass to find the empirical formula of a hydrate. In this lab and unknown hydrate will be heated two separate times over a Bunsen burner to remove as much water from the substance as possible, before and after heating the crucible the masses will be calculated and recorded for future reference. To participate in this lab it is important to know he formulas that will be worked with. The formula of the hydrate that will be used, Copper II Sulfate, is CuSo4 • 5H2O. Along with this, the formula used to calculate the percent water in the hydrate will

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

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

Can the concentration of hydrochloric acid increase the rate of the reaction between magnesium ribbon and hydrochloric acid?

One error for the experiment could be from the popping and spritzing of the hydrate when heating it, which could have caused a slight decrease in mass of the whole compound. Since some of the hydrate spritz out of the crucible, the mass decreased. This directly affected the results of the experiment because the mass that spritzed out of the crucible caused the mass to be weighted differently when remeasured on the scale. Another error of the experiment was that there was some hydrate that stuck to the stirring rod when stirring the hydrate.

Fill the crucible halfway with the unknown hydrate. Measure and record the mass of the crucible and the hydrate.

We were also provided with 6 molar following reagents:  H2SO4  HCl  NH3  NaOH Experimental Methods: We adopted these steps to find out the formula of unknown hydrate: Qualitative analysis: The unknown hydrate (in solution form) was reacted with all given known aqueous solution and reagents separately in separate test tubes and results were noted down in Table No. 1.1. Quantitative Analysis: The number of water molecules were determined by following steps: o Determined the mass of water that has left the compound.

Dissolve 40g povidone in 120g water. Blend 200g lactose, 4g Blue#1, 0.8g Yellow #10. Screen rough blend for clumps and blend to uniform color. Add povidone solution to povidone and 515.2g lactose to granulate. Add water to appropriate consistency, then dry product to specification. Sift material to correct fleck size (wet granulation of coating). Blend 450g of sodium glycolate to 20g silicon dioxide. Screen material. Blend 2700g starch, 7980g MC, 50g Mg stearate, 800g of blue granulation (above) (press coating). For the core, blend 2675g cyclophosphamide monohydrate to 5g silicon dioxide, blend with 1150g starch, 150g starch glycolate, and 20g magnesium stearate. Compress core, then surround core with coating by second direct compression. Hardness

Nausea and vomiting: Early signs of magnesium deficiency can include gastrointestinal discomfort such as nausea and vomiting

Studies show that as many as half of all Americans do not consume enough magnesium. Magnesium deficits have been tied to allergies, asthma, attention deficit disorder, anxiety, heart disease, muscle cramps and other conditions.

To the different part of the lab was to identify the melting points of the vanillin. First, slightly less than 30 mL of water and a stir bar was added into a clean flask. Two capillary tubes were needed for contaminated vanillin and recrystallized vanillin. For each of the capillary tube, small bits of contaminated vanillin crystal was scooped into the capillary tube and a tiny bit of recrystallized vanillin was scooped into the another capillary tube. After both capillary tubes had to be labeled, that way it was much easily to remember which one which. Then, the flask was placed on the burner. Before the burner was turned on, the thermometer had to be measured inside the flask within the water. And attached with a rubber ring, two capillary