03.09 Molar Mass of Compounds: Determining the Formula of a Hydrate
[ print page ]03.09 Molar Mass of Compounds: Determining the Formula of a Hydrate—Text Version
When hydrates are heated, the water of hydration evaporates and is released as vapor. The remaining solid is known as the anhydrous salt, which is the compound same compound without the water molecules trapped inside.
Title:The title of the lab should be at the top of the lab report.
Purpose: In one or two complete sentences, state the purpose of this laboratory investigation.
Materials: List all of the materials (balance, crucible, etc.) used in this lab
Procedure:Include a step-by-step procedure for what you did in the lab, written in your own words
Data and Observations:Be sure that all measurements have the correct number of sig-figs and the correct units
Mass, grams Mass of empty crucible Mass of crucible and hydrate Mass of hydrate Mass of crucible and dehydrate Mass of dehydrate
Also include any observations (not measured) that you made during the course of the investigation.
Calculations:1.Obtain the mass of the empty crucible. Obtain the mass of the crucible and the hydrate. Subtraction of the mass of the empty crucible from the mass of the hydrate and crucible gives the mass of the CuSO4 hydrate.
Mass of hydrate = (mass of crucible + hydrate) - (mass of empty crucible)
2.Heat the hydrate. After heating, record the mass of the crucible and the dehydrated compound.
No calculations for this step
3.Subtracting the mass of the empty crucible from the mass of the crucible and dehydrated CuSO4 gives you the mass of the dehydrated compound.
Mass of dehydrate = (mass of the crucible and dehydrated) - (mass of empty crucible)
4.Subtract the mass of the dehydrated compound from the mass of the hydrate to determine the mass of water that was present in the hydrate.
Mass of water = Mass of hydrate - mass of dehydrate
5.Convert the mass of water to moles of water.
6.Convert the mass
When hydrates are heated, the water of hydration evaporates and is released as vapor. The remaining solid is known as the anhydrous salt, which is the compound same compound without the water molecules trapped inside.
Title:The title of the lab should be at the top of the lab report.
Purpose: In one or two complete sentences, state the purpose of this laboratory investigation.
Materials: List all of the materials (balance, crucible, etc.) used in this lab
Procedure:Include a step-by-step procedure for what you did in the lab, written in your own words
Data and Observations:Be sure that all measurements have the correct number of sig-figs and the correct units
Mass, grams Mass of empty crucible Mass of crucible and hydrate Mass of hydrate Mass of crucible and dehydrate Mass of dehydrate
Also include any observations (not measured) that you made during the course of the investigation.
Calculations:1.Obtain the mass of the empty crucible. Obtain the mass of the crucible and the hydrate. Subtraction of the mass of the empty crucible from the mass of the hydrate and crucible gives the mass of the CuSO4 hydrate.
Mass of hydrate = (mass of crucible + hydrate) - (mass of empty crucible)
2.Heat the hydrate. After heating, record the mass of the crucible and the dehydrated compound.
No calculations for this step
3.Subtracting the mass of the empty crucible from the mass of the crucible and dehydrated CuSO4 gives you the mass of the dehydrated compound.
Mass of dehydrate = (mass of the crucible and dehydrated) - (mass of empty crucible)
4.Subtract the mass of the dehydrated compound from the mass of the hydrate to determine the mass of water that was present in the hydrate.
Mass of water = Mass of hydrate - mass of dehydrate
5.Convert the mass of water to moles of water.
6.Convert the mass