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?
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
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).
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
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
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
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
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
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
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)
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