Part A Part complete Part B Part complete You dry the hydrate as instructed in t

Question

Part A

Part complete

Part B

Part complete

You dry the hydrate as instructed in the lab procedure, noting down it's mass until it appears to no longer decrease (no more water bound in the sample).

Part C

Part complete

So what is the Mass of Water (liberated during drying)?
(DO NOT put units: grams is assumed)

Part D

How many Moles of Anhydrous Salt is this (moles of CuSO4)?
(DO NOT put units: moles is assumed)

Part E

Part complete

How many Moles of Water were in the sample (liberated during heating)?
(DO NOT put units: moles is assumed)

Part A

Part complete

Based on the following data, complete the table below as if you were making the calculations described in the lab.
Formula of Anhydrous Salt (supplied by instructor) CuSO4 Mass of Crucible 26.30 g Mass of Crucible + Hydrate 29.75
What is the mass of Hydrate in grams?
(DO NOT put units: grams will be assumed)

Part B

Part complete

You dry the hydrate as instructed in the lab procedure, noting down it's mass until it appears to no longer decrease (no more water bound in the sample).

Mass of Salt + Crucible (after 1st heating) 28.57 Mass of Salt + Crucible (after 2nd heating) 28.51
What is the Mass of Salt after second heating (ie. dry CuSO4)?
(DO NOT put units: grams is assumed)

Part C

Part complete

So what is the Mass of Water (liberated during drying)?
(DO NOT put units: grams is assumed)

Part D

How many Moles of Anhydrous Salt is this (moles of CuSO4)?
(DO NOT put units: moles is assumed)

Part E

Part complete

How many Moles of Water were in the sample (liberated during heating)?
(DO NOT put units: moles is assumed)

Explanation / Answer

(A)

Mass of Hydrate = 29.75 - 26.30 = 3.45 g.

(B)

Mass of salt after first heating = 28.57 - 26.30 = 2.27 g.

Mass of salt after second heating = 28.51 - 26.30 = 2.21 g.

(C)

Mass of water = 3.45 - 2.21 = 1.24 g.

(D)
Mass of anhydrous salt = 2.21 g.

Moles of anhydrous salt = 2.21 / (63.5 + 32 + 64) = 0.0138 mol

(E)

Moles of water = 1.24 / 18 = 0.0689 mol

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