Question 1001501
The website yeahchemistry.com will help you with chemistry questions.
If the solution was 100% sulfuric acid, you would have 500g sulfuric acid and 0g water.
When you buy a bottle of sulfuric acid it would have a label with analysis data,
and it could read "assay = 98.6%", or something like that.
However, you may assume, it is 100%, because 1.84g/mL is the densityof 100% sulfuric acid at {{{10^o}}} .
(Warmer acid, and/or less concentrated acid has a lower density).
Then, {{{(500g)*(1mol/"98 g")=5.1mol}}} would give you the number of moles of sulfuric acid.
You can use the density to find the volume of those 500g solution,
{{{500g*(1mL/1.84g)=272mL=0.272L)}}} .
Then, {{{5.1mol/"0.272 L"=18.8}}}mol/L is the molarity, often written as {{{18.8M}}} , and read as "18.8 molar".
Since {{{500g=0.5kg}}} , {{{5.1mol/"0.5 kg"=10.2}}}mol/kg is the molality,
which your instructor may express as {{{10.2molal}}} or {{{10.2m}}} .
The mole fraction would be
moles acid/{moles acid + moles water) ,
and since we are assuming 0% water,
that molar fraction would be {{{1.0"}}} .