# chemistry

In the experiment, a hydrate is heated to form an anhydrate. The masses of the before and after are measured and the percent of the water in the hydrate is calculated. If some of the hydrate spatters out of the crucible and isnt noticed, how will this affect the calculated percent of the water in the hydrate?

1. 0
2. 13
1. You have less mass when you weigh it, so the apparent mass of the hydrate will be less, so the apparent mass of the water will be greater.

1. 0
posted by bobpursley
2. This will decrease the second measurement, the mass of the anhydrate. Therefore, it will seem like more water evaporated, thus this will increase the apparent percent of water in the hydrate, leading you to believe the hydrate had more waters of hydration

1. 0
posted by Ryan
3. you beat me to it

1. 0
posted by Ryan
4. will the anhydrous mass be less as well?

1. 0
posted by sylvia
5. I assume you are only measuring the total weight of the system each time. So on the second measurement you assume that you have completely dehydrated the anhydrate. So you can't tell if you actually lost any anhydrate (unless you know you did).

1. 0
posted by Ryan
6. A similar thing happened to me !!!!! thanks for the help

1. 0
7. And Btw - for me we had to find the emperical formula for CuSO4 . H2O and after doing the experiment I found out that the value that i got was CuSO4 . 6H2o when the correct answer should be CuS04 . H2o

1. 0

## Similar Questions

1. ### Chemistry

Predict the effect of each of the following by mass of water in the hydrate and the chemical of the hydrate? a) not heating the hydrate enough b) overheating the hydrate and producing some copper (ii) oxide C) the initial hydrate
2. ### Chemistry

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
3. ### 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
4. ### Chemistry

An unknown hydrate of copper (II) oxalate is to be identified in the lab. The following data was collected by a student: Mass of crucible 23.776 g Mass of crucible + hydrate 24.889 g Mass of crucible + anhydrate 24.530 g Thank you
5. ### 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.
6. ### 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.
7. ### Chemistry

During your experiment, you are drive water from the hydrate M x X y ⋅zH 2 O . You subsequently determine that your hydrate has four molecules of waters associated with each formula unit. However, the bottle the hydrate came
8. ### 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)
9. ### Chemistry

During your experiment, you are drive water from the hydrate MxXy*zH2O. You subsequently determine that your hydrate has six molecules of waters associated with each formula unit. However, the bottle the hydrate came from
10. ### Chemistry

A 5 gram sample of a hydrate of BaCL2 was heated, and only 4.3g of the anhydrous salt remained. What percentage of water was in the hydrate?

More Similar Questions