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~angel~
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I just wanted to see if I'm doing this right.
Sulfuric acid is supplied as a concentrated liquid. A bottle was assayed and found to have a density of 1.84 g/mL and a purity of 97%. The molecular weight of H2SO4 is 98. What is the molarity of this solution?
molarity=moles/volume
moles=mass/mol.weight
moles=1.84/98
moles=1.88*10^-2
assuming the volume is 1mL=0.001L,
molarity=1.88*10^-2/0.001
molarity=18.80 mol/L
since there is 97% purity,
molarity=18.80*0.97
=18.24 mol/L
Is this right? I think I'm wrong, but this was just a guess.
Thanks.
Sulfuric acid is supplied as a concentrated liquid. A bottle was assayed and found to have a density of 1.84 g/mL and a purity of 97%. The molecular weight of H2SO4 is 98. What is the molarity of this solution?
molarity=moles/volume
moles=mass/mol.weight
moles=1.84/98
moles=1.88*10^-2
assuming the volume is 1mL=0.001L,
molarity=1.88*10^-2/0.001
molarity=18.80 mol/L
since there is 97% purity,
molarity=18.80*0.97
=18.24 mol/L
Is this right? I think I'm wrong, but this was just a guess.
Thanks.