Posted by **Beth** on Tuesday, January 5, 2010 at 10:24pm.

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.

- AP Chemistry -
**DrBob222**, Wednesday, January 6, 2010 at 12:05am
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.

- AP Chemistry -
**Anonymous**, Friday, June 6, 2014 at 1:01pm
volume of 34.6 and mass of 46.0 what is the SF

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