Hydrate Formula
Muhil Arumugam
Gold 3 Calculating the Formula of a Hydrate through Experimentation Purpose
The purpose of this lab is to determine the formula of a given hydrate through collecting and calculating experimental data.
Data
Mass (g) of crucible
29.9g
Mass (g) of crucible with hydrate
32.35g
Mass (g) of crucible and anhydrous salt
31.39g
Questions and Calculations
1. What was the mass of the original hydrate?
2.45g of hydrate
Calculations: Mass of crucible with hydrate (32.35g) - Mass of crucible (29.9g) = 2.45g
2. Calculate the mass of water lost from the hydrate.
.96g of water lost from hydrate
Calculations: Mass of crucible with hydrate (32.35g) - Mass of crucible and anhydrous salt (31.39g) = .96g
3. How many moles of water is this? …show more content…
This is supported by the experimental data collected from the experiment. From our data, it can be easily calculated that the mass of the lost water was .96g and the anhydrous salt left behind massed at 1.49g. Using this information it can be determine the moles of each substance (.96g/18.02g=.053 moles of water, and 1.49g/159.62=.00933 moles of anhydrous salt). This is possible to calculate due to the scientific understanding that the mass of an element in grams divided by its average atomic mass will calculate the moles it’s equivalent to. After calculating the moles of each, the ratio .053 moles of water to .00933 moles of anhydrous salt is formed. Then, by dividing the moles of water by the moles of anhydrous salt a ratio between the two will be formed. This is because of a scientific principle that when dividing the moles of one molecule by another will result in a proportion of moles of one element to 1 mole of the other. The calculation produces 5.6806 moles of water/1 mole of anhydrous salt and after rounding to the nearest whole number the ratio 6 moles of water to 1 mole of anhydrous salt forms. Last, when plugged into the chemical formula of the hydrate (copper (ii) sulfate), the result is 1CuSO46H2O, which is the formula of the
Gold 3 Calculating the Formula of a Hydrate through Experimentation Purpose
The purpose of this lab is to determine the formula of a given hydrate through collecting and calculating experimental data.
Data
Mass (g) of crucible
29.9g
Mass (g) of crucible with hydrate
32.35g
Mass (g) of crucible and anhydrous salt
31.39g
Questions and Calculations
1. What was the mass of the original hydrate?
2.45g of hydrate
Calculations: Mass of crucible with hydrate (32.35g) - Mass of crucible (29.9g) = 2.45g
2. Calculate the mass of water lost from the hydrate.
.96g of water lost from hydrate
Calculations: Mass of crucible with hydrate (32.35g) - Mass of crucible and anhydrous salt (31.39g) = .96g
3. How many moles of water is this? …show more content…
This is supported by the experimental data collected from the experiment. From our data, it can be easily calculated that the mass of the lost water was .96g and the anhydrous salt left behind massed at 1.49g. Using this information it can be determine the moles of each substance (.96g/18.02g=.053 moles of water, and 1.49g/159.62=.00933 moles of anhydrous salt). This is possible to calculate due to the scientific understanding that the mass of an element in grams divided by its average atomic mass will calculate the moles it’s equivalent to. After calculating the moles of each, the ratio .053 moles of water to .00933 moles of anhydrous salt is formed. Then, by dividing the moles of water by the moles of anhydrous salt a ratio between the two will be formed. This is because of a scientific principle that when dividing the moles of one molecule by another will result in a proportion of moles of one element to 1 mole of the other. The calculation produces 5.6806 moles of water/1 mole of anhydrous salt and after rounding to the nearest whole number the ratio 6 moles of water to 1 mole of anhydrous salt forms. Last, when plugged into the chemical formula of the hydrate (copper (ii) sulfate), the result is 1CuSO46H2O, which is the formula of the