# Chemistry

I need help with this lab.

Write the equation for the decomposition of the hydrate, CuSO4*XH2O.

Mass of crucible and hydrate: 93.000g
Mass of crucible and pure salt: 91.196g

I need to calculate the following:

1. mass of water in hydrate sample(g)
2. number of moles of water in the sample
3. mass of pure salt in the sample(g)
4. number of moles of salt in the sample
5. molar ratio of water to salt in the sample

From your calculations what is the empirical formula of copper sulfate hydrate?

I cant figure out how to get the emperical formula??????

1. 👍 0
2. 👎 0
3. 👁 243
1. If you have no more data than this I can't figure it out either.

93.000 g = mass xble + hydrate
91.196 g = mass xble + salt
---------
1.804g = mass water lost
mols H2O = 1.804/18 = 0.100

But this is as far as you can go.
You need the mass of the crucible, then you can figure the mass of the CuSO4.
mols CuSO4 = grams/molar mass.

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chemistry

I don't understand these two questions. Any help on how to figure this would be great. Thanks. 1. Write the equation for the decomposition of the hydrate, MgC*XH₂O 2. Write the equation for the decomposition of the hydrate,

asked by Matt on February 15, 2010
2. ### chemistry

I need help with this lab. Write the equation for the decomposition of the hydrate, CuSO4*XH2O. Mass of crucible and hydrate: 93.000g Mass of crucible and pure salt: 91.196g I need to calculate the following: 1. mass of water in

asked by Nancy on November 8, 2012
3. ### Chemistry :/

Experiment 1 results: mass of crucible 88g mass of hydrate 93g mass of salt 91.196g 1. Calculate the following: a:mass of water in the hydrate sample (g) b:number of moles of water in the sample c:mass of pure salt in the sample

asked by Leanna on March 7, 2015
4. ### chemistry

If a 8.6195 g of a mixture which contains (20.0 % of CuSO4.XH2O and 80.0 % of sand) was heated in a crucible then cooled in the desiccator the mass obtained was 7.9976 g. a- Find X the number of water of hydration in the Hydrate

asked by Janaiby on July 15, 2013
5. ### Chemistry

Experiment 1 results: mass of crucible 88g mass of hydrate 93g mass of salt 91.196g 1. Calculate the following: a:mass of water in the hydrate sample (g) b:number of moles of water in the sample c:mass of pure salt in the sample

asked by Leanna on March 7, 2015
6. ### Chemistry

A hydrate of copper (II) sulfate with formula CuSO4.xH2O has a molar mass of 250.0 g/mol. 2.545 g of hydrate is heated and 63.85% of the residue is found after heating. a) Determine the value of x in the formula of the compound b)

asked by Kai on June 17, 2017
7. ### Chem 11

So I did a lab determining the chemical formula of a hydrate. I really just need somebody to check this over for me. We had to find the molecular formula of a hydrate of copper (2) sulphate, CuSO4 .xH2O. My observation table looks

asked by Katherine on November 18, 2014
8. ### Chemistry 11

So I did a lab determining the chemical formula of a hydrate. We had to find the molecular formula of a hydrate of copper (2) sulphate, CuSO4 .xH2O. My observation table looks like this: Mass of clean, dry test tube: 21.6g Mass of

asked by Katherine on November 18, 2014
9. ### Chemistry

Is the decomposition equation for copper sulphate hydrate (CuSO4.5H2O) as follows: CuSO4+5H2O? Thanks

asked by Emma on October 21, 2009
10. ### Chemistry

Hi I need with with a prelab calculation for a Hydrate Crystal lab and I am so confused @_@ You don't really need to solve it if you don't want to, I just need an example on how to do these problems 1) Find the mass of the water

asked by Sira on October 11, 2012

More Similar Questions