03.09 the formula of the hydrate.Data and Observations-

03.09 Molar Mass of Compounds: Lab Report OutlineTitleTo Determine  the Formula of a HydratePurposeI performed the experiment in order to determine the formula of a copper sulfate hydrate by heating the sample until the water evaporates.Materials- Scale- Balance- Crucible- Hydrate- Bunsen BurnerProcedureFirst you measure the mass of the empty crucible and record that mass. Then you should fill theCrucible with 3-5 scoops of the hydrate and record that mass as well. Heat the hydrate filledCrucible above the Bunsen burner for 10 minutes for all of the water to evaporate. Let the cruciblecool and then mass the crucible with dehydrated solid inside. Record that mass and finallycalculate the formula of the hydrate.Data and Observations- Mass of empty crucible- 19.508g- Mass of crucible and hydrate- 40.014g- Mass of hydrate- 20.506g- Mass of crucible and dehydrate- 40.038g- Mass of the dehydrate- 20.530g- Before I heated the hydrate, the color of the hydrate was blue. When I started heating the hydrate over the Bunsen burner the color changed from blur to white and stayed the same after cooling.Calculations1. Get the mass of the empty crucible. Then obtain the mass of the crucible and the hydrate.After that, we will have to subtract the mass of the empty crucible from the mass of the hydrate and that gives you the mass of the CuSO4 hydrate which is 20.530g.2. Heat the hydrate, once it is heated, note down the mass of the crucible and the dehydrated which is 20.447g3. Then we will subtract the mass of the crucible and the dehydrated Copper Sulfate with the mass of empty crucible which is 20.530g then we will subtract the amount with the mass of crucible again which will give us the mass of dehydrate mass which is 1.022g4. We will subtract the mass of the dehydrate CuSO4 which was calculated in step 3 from the mass of the hydrate to determine the mass of water that was present in the hydrate which is 19.484g5. Then we will convert the mass of water to moles of water and it will give us 1.0815 moles6. We will also convert the mass of dehydrated CuSO4 to moles of the compounds and it will give us 1.139 moles7. Divide by the lowest mole value to get a whole number mole ratio which will give us 18 (9×2=18). The mole ratio is 0.007Which will give us the formula: CuSO4*9H20Discussion and Conclusion:The first part of this section of the lab is the discussion, in which you discuss any mistakesthat may have been made (or what measures were taken to try to avoid mistakes) and whatimprovements, if any, you can think of for the procedure for the next time the lab will beconducted.? In the discussion section of this lab report, you will want to discuss the importance forheating the hydrate for a sufficient amount of time. Also address the followingquestions in your discussion:?1. How would you expect the final measured mass of the anhydrate to change ifthe hydrate was not heated for a sufficient length of time, and why??The compound is heated for a sufficient amount of time so that it isn’t over heated or under heated. Basically to perform the experiment without any error, or being biased.2. How would this change in the measured final mass affect the calculatedformula of the hydrate? Explain your answer to these questions thoroughly. I don’t think there will be a dramatic change in the final mass. If it were to be heated for a sufficient amount of time it would be wet, and still be a hydrate, and it would weigh more than a hydrate compound.? A conclusion is usually a paragraph that sums up what was done in the lab and whatthe findings or results are.In the experiment, I determined the formula of Copper Sulfate hydrate by heating it until the water evaporates. This experiment included five steps in order to find the formula. After completing all five steps; I had to calculate the formula of Copper Sulfate II. Consequently, I found the mass and mole of th