ProficientWriting | Formula, and molar mass of your hydrate sample

Formula, and molar mass of your hydrate sample

What was the name, formula, and molar mass of your hydrate sample? (1.5 pts)
The name of the given hydrate sample for our group is iron sulfate. Iron sulfate has a formula of FeSO4
.
The molar mass of the hydrate sample is 151.908 g/mol.
Write the general equation for your dehydration reaction for your specific salt. (Hint: you don’t
know how much water was lost yet so you should have a variable in the equation)(2 pts)
FeSO4

Calculate the mass of the metal salt product with no water molecules. (Hint: Use dimensional
analysis and your drying equation, this would be a complete dehydration reaction) (4 pts)
Using the previous answer, calculate the mass of water remaining in the sample. Did your sample
dry completely? (1 pt)
What is the mass of water lost by heating? (1 pt)
Report the mass of metal salt, the mass of water lost, and the mass of water left in moles. (1.5pts)
Write out the experimentally determined equation associated with your hydrate salt. (2 pts)
What is the name of your final hydrate salt? (1 pt)
Compare your data to those of your classmates with the same starting material. How were your
answers similar? How were they different? (2 pts)
Discuss the limitations of your data and/or ways that the experiment could be improved. (2 pts)

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