Asked by Beth

An aqueous sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution at 20°C has a density of
1.3294 g/mL. Calculate (a) the molarity, (b) the molality, (c) the percent by mass, and (d) the mole fraction of
H2SO4 for the solution. (MM H2SO4 = 98.08; MM H2O = 18.01

I have no idea where to start.
Answered by DrBob222
You must remember the definitions. I'll get you started.
M = #moles/liter of solution.
m = # moles/kg solvent.
%w/w = grams H2SO4/100 g solution.
X = moles H2SO4/(moles H2SO4 + moles H2O)

For the first one, molarity.
density = 1.3294 g/mL.
So how much would a liter weigh? It will weigh 1.3294 g/mL x 1000 mL = 1329.4 grams.
How much of that is H2SO4? The problem tells you it has 571.6 g H2SO4 in it.
How many moles is that? It is
571.6 g H2SO4 x (1 mole H2SO4/98.08 g H2SO4) = 5.8279 moles which rounds to 5.828 to 4 significant figures.
So you have 5.828 moles H2SO4/L of solution which makes it 5.828 molar.

I will leave the others to you. Just follow the definitions.
Answered by Anonymous
volume of 34.6 and mass of 46.0 what is the SF
Answered by suresh
The molality is equal to 0.0045146727
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