1. Chemistry
2. Physical Chemistry
3. Energetics and Thermodynamics
4. 17705

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1. Given that moles of water loss = Weight of water / GMW H2O (=18.051 ) and moles of CuSO4 = final weight/ GMW CuSO4 (=159.61)

:Initial Weight: 116.877g (cooper II sulfate hydrate 30g + water )

:Final Weight: 19.177g (after heat compound with burner)

:Weight of Water driven off (Initial weight - final weight) : 97.7g

X = moles of water loss/ moles of CuSO4
Given that hydrate is: CuSO4 (XH2O)

What is the formula of the hydrate?

2. Given that initial unknown chloride sample weight (g): 5g, and Weight of AgCl precipitate: 21.987g, and approximate volume of AgNO3 solution added (ml): 1M

What is
Moles of AgCl = ( AgCl precipitate mass/143.32 ):
Weight of Cl- in XCl sample = (moles of AgCl)x(atomic weight of Cl- = 35.4527) :
% Cl- in sample = (weight of Cl- in XCl sample / weight of XCl sample) x 100 % :

What happened as excess AgNO3 solution was added to the XCl solution?