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.

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.

volume of 34.6 and mass of 46.0 what is the SF

To solve this problem, you need to understand the concepts of molarity, molality, percent by mass, and mole fraction. Let's break down each calculation step-by-step.

(a) Molarity (M):

Molarity is defined as the number of moles of solute per liter of solution. In this case, the solute is H2SO4. The given information states that the solution contains 571.6 g of H2SO4 per liter of solution.

1. To find the moles of H2SO4, divide the given mass by the molar mass of H2SO4.
Moles of H2SO4 = mass of H2SO4 / molar mass of H2SO4

Moles of H2SO4 = 571.6 g / 98.08 g/mol

2. Now, divide the moles of H2SO4 by the volume of the solution (which is 1 liter) to find the molarity.
Molarity = moles of H2SO4 / volume of solution (in liters)

Molarity = (571.6 g / 98.08 g/mol) / 1 L

Now, you can calculate the molarity of the solution.

(b) Molality (m):

Molality is defined as the number of moles of solute per kilogram of solvent. In this case, the solvent is water (H2O).

1. To find the moles of H2SO4, divide the given mass by the molar mass of H2SO4 (same as step 1 in part a).

2. Since the molality requires the mass of the solvent, we need to calculate the mass of water.

Mass of water = mass of solution - mass of H2SO4
Mass of water = 1000 g (1 liter) - 571.6 g

3. Convert the mass of water to kilograms.
Mass of water = (1000 g - 571.6 g) / 1000 g/kg

4. Now, divide the moles of H2SO4 by the mass of water (in kg) to find the molality.
Molality = moles of H2SO4 / mass of water (in kg)

(c) Percent by mass:

Percent by mass is the ratio of the mass of the solute to the mass of the solution multiplied by 100.

1. Calculate the mass of H2SO4 in the solution (same as step 1 in part a).

2. Calculate the mass of the solution by multiplying the density (given as 1.3294 g/mL) by the volume (1 L).

Mass of solution = density × volume

Mass of solution = 1.3294 g/mL × 1000 mL

3. Now, divide the mass of H2SO4 by the mass of the solution (both in grams) and multiply by 100 to find the percent by mass.

Percent by mass = (mass of H2SO4 / mass of solution) × 100

(d) Mole fraction:

Mole fraction is the ratio of the moles of a component to the total moles of all components in the solution.

1. Calculate the moles of H2SO4 (same as step 1 in part a).

2. Calculate the moles of water by dividing the mass of water by the molar mass of H2O.
Moles of water = mass of water / molar mass of H2O

3. Calculate the total moles by summing the moles of H2SO4 and moles of water.

4. Calculate the mole fraction of H2SO4 by dividing the moles of H2SO4 by the total moles.

Now you can apply these steps to calculate the values of (a) the molarity, (b) the molality, (c) the percent by mass, and (d) the mole fraction of H2SO4 for the solution.

The molality is equal to 0.0045146727