First we calculate the formula mass of the compound magnesium sulfate.Formula mass of MgSO4 = 24.3 + 32.1 + 4(16.0) = 120.4
Amount of MgSO4 in a 480g pure sample = 480/120.4 = 3.99mol
There is approximately 4 moles of the compound present in a 480g sample.
2
Aluminium Sulphate is Al2(SO4)3 and its mass is27x2 + 96x3 = 342g/mole
0.125 Molar solution! Molarity = moles of solute/Liters of solution Algebraically manipulated, Moles of copper sulfate = 2.50 Liters * 0.125 M = 0.313 moles copper sulfate needed ===========================
Molar mass of MgCl2 is 95gmol-1. So there are 0.566 moles in this mass.
1,25 g of anhydrous iron(III) nitrate = 0,005 moles
The answer is approx. 2 moles (for anhydrous sodium sulfate).
1020g
4,12 grams aluminum sulfate is equivalent to 0,012 moles (for the anhydrous salt).
Depends on if it is hydrated or not. If hydrated, magnesium sulfate heptahydrate, then (7.6g)/(246.47g/mole)=.0308mole. If anhydrous (7.6g)/(120.415g/mole)=0.063mole.
9 g anhydrous magnesium nitrate = 0,061 mol
molec weight is 151g/mol. 1.11 moles x 151g/mol is 167.61g Moles is mass / molecular mass
The molar mass of anhydrous sodium sulfate is 142,04.
9
6,8 x 95,211 g (molar mass of anhydrous MgCl2)The mass of 6.80 moles of magnesium chloride or MgCl2 is 647,435 g.
5,7 moles (SO4)3-.
2
1,125 moles of sodium sulfate contain 6,774908464125.10e23 molecules.