mass of H2O = mass of hydrated salt - mass of anhydrous salt
mass of H2O = 1.687 g - 0.824 g
mass of H2O = 0.863 g
Molar mass of H2O,
MM = 2*MM(H) + 1*MM(O)
= 2*1.008 + 1*16.0
= 18.016 g/mol
mass(H2O)= 0.863 g
use:
number of mol of H2O,
n = mass of H2O/molar mass of H2O
=(0.863 g)/(18.02 g/mol)
= 4.79*10^-2 mol
Molar mass of MgSO4,
MM = 1*MM(Mg) + 1*MM(S) + 4*MM(O)
= 1*24.31 + 1*32.07 + 4*16.0
= 120.38 g/mol
mass(MgSO4)= 0.824 g
use:
number of mol of MgSO4,
n = mass of MgSO4/molar mass of MgSO4
=(0.824 g)/(1.204*10^2 g/mol)
= 6.845*10^-3 mol
use:
X = mol (H2O)/mol (MgSO4)
X = 4.79*10^-2 / 6.845*10^-3
X = 7
Answer: 7
If "Epsom salt," MgSO4 x H2O is heated to 250°C. all the water of hydration is...
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A 6.2351 g sample of an unknown hydrate of cobalt(II) bromide is heated until all the water of hydration is removed. The CoBr2 that remains has a mass of 5.0000 g. 1. How many moles of CoBr2 are in the sample? mol 2. How many grams of water were lost in the dehydration? g 3. How many moles of water were lost? (mol) 4. What is the value of "n" in the formula CoBr2 · n H2O? (1, 2, 3,...
determining the formula of a hydrate of calcium chloride (CaCl2·X H2O). Mass (g) Crucible and Lid 28.4735 Crucible and Lid + hydrate salt 33.1938 Crucible and Lid + anhydrous residue 32.0339 What is the mass of the hydrate? mass = ___ g What is the mass of the anhydrous residue? mass = ___ g What is the mass of water lost upon heating the sample? mass = ___ g How many mol of H2O were lost upon heating? (H2O: 18.016...
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