# Chemistry

posted by .

After 0.6523 g of CoCl2*6H2O is heated, the residue has a mass of 0.3423 g. Calculate the % H20 in the hydrate. What is the formula of the hydrate?

-I understand how to get the % H2O in the experiment but how do you determine the formula?

• Chemistry -

There are two or three ways to do it but this is what I do.
0.6523 - 0.3423 = 0.3100 g = mass H2O.
mols H2O = 0.3100/18 = 0.01721
mols CoCl2 = 0.3423/129.838 = 0.00264.

Mow you want the ratio of mols H2O to 1 mol CoCl2; therefore, let's MAKE CoCl2 1. How do we do that. Divide the mols CoCl2 by itself; i.e., 0.00264/0.00264 = 1.000
Then H2O must be treated the same way so that is 0.01721/0.00264 = 6.53 which rounds to 6.5 and the formula would be CoCl2*6.5H2O or 2CoCl2*13H2O.
I think most of the CoCl2 I read about is CoCl2*6H2O (although there are several different hydrates). Is this an experiment and you have typed in your experimental data? That might explain the funny number. If this is a problem you have been given, please check the numbers to make sure they were typed in correctly. Check my arithmetic to make sure I didn't make an error.

• Chemistry -

Convert the mass of dry residue, CoCl2, to moles by dividing it by the formula mass of CoCl2.
Determine the mass of water (loss in mass of sample).
Convert grams of H2O to moles by dividing by its formula mass.
Determine the mole ratio of H2O/CoCl2:
(moles H2O) / moles (CoCl2)
Your ratio is somewhat higher than the correct ratio of 6.

• Chemistry -

Well what I did to get the % H2O is just subtract the end product(0.3423)from the original sample (0.6523) to get the 0.3100 H20 then found the percent by dividing and got 47.5% H20. Is this the completely wrong method of going about this problem and should do the moles way?

• Chemistry -

No, your work is ok for the percent water. Since you told us in the problem that you already knew how to do that, neither GK nor I addressed the percent part of the problem but went straight to the determination of the formula. By the way, I calculate 47.5% H2O also. You can avoid all of the small numbers (like I used) in the determination of the formula if you take a 100 g sample. That gives you 47.5 g H2O and 52.5 g CoCl2. Then convert those grams to mols and obtain the formula that way. You'll still end up with CoCl2*6.5H2O which is slightly high. I assume these are experimental data.

• Chemistry -

A sample of CoCl2 XH2O with a mass of 1.62g was heated. After heating only 0.88 of CoCl2 remained. Determine the name and formula for the hydrate.

## Similar Questions

1. ### chem

A 3.48 gram sample of sodium sulfate hydrate lost 1.35 gram of water when heated to constant weight. What is the formula of the hydrate?
2. ### Chemistry

After 0.6523 g of is heated, the residue has a mass of 0.3423 g. Calculate the % H2O in the hydrate.
3. ### chemistry

A 2.50 g sample of a hydrate of calcium sulphate losses 0.523 g of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
4. ### chemistry

A 2.500 gram sample of hydrate of calcium sulfate loses 0.532 grams of water when heated. Determine the mass percent of water in the hydrate and the formula of the hydrate.
5. ### science

After 0.6523 g of CoCl_{2} \cdot 6H_{2}O is heated, the residue has a mass of 0.3423 g. Calculate the % H2O in the hydrate.
6. ### Chemistry

1.62 g of CoCl2 x (xH20) were heated. After heating only .88g of CoCl2 remained. What was the formula of the original hydrate?
7. ### Chemistry

A 32.907-g sample of a hydrate of Au (CN)3 contains 5.406 g H2O What is the formula for the hydrate?
8. ### chemistry

Cobalt(2) chloride is commonly obtained from chemical supply houses as a hydrate with the formula COCL2*6H2O an analysis showed that 25.0 g of this hydrate contains 11.3 g of water what is the percent water by weight in this hydrate?
9. ### Chemistry

7. A student conducts an experiment on a different hydrate. The empty crucible is heated to a constant mass of 24.330. A sample of the unidentified hydrate is placed in the crucible, and the total mass is 31.571 g. The crucible and …
10. ### 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) …

More Similar Questions