Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: dnellie on December 07, 2012, 02:55:02 PM
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concentrated sulfuric acid is 95% H2SO4 by mass with the balance of the mass being made up of water. The density of concentrated H2SO4 is 1.84 g/cm^3. i need to determine the molarity and molality of H2SO4. In class we only determined these values for solutes but in this case isn't H2SO4 a solvent? do i still use the same equations.
i know these equations
M=moles of solute/ Liters of solution
m=Moles of solute/kg solvent
but what i don't understand is what are these giving me the molarity and molality of the solute, the solvent or the solution.
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In class we only determined these values for solutes but in this case isn't H2SO4 a solvent?
No.
H2SO4 = solute.
H2O=Solvent
Though can be confusing since the solution is commonly called "H2SO4" as well.
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In class we only determined these values for solutes but in this case isn't H2SO4 a solvent?
No.
H2SO4 = solute.
H2O=Solvent
Though can be confusing since the solution is commonly called "H2SO4" as well.
thank you