A commertially available sample of H2SO4 is 15% of H2SO4 by weight. Density=1.10g. Calculate-

1. Molarity
2. Normality
3. Molality

Wonder who would offer that as a "sample"?

Molarity: grams/molmass*volumeInLiters
so if you had one liter of this stuff, you so assume 1 liter of this stuff, which is 1100g

.15*1100/98*1=165/98 Moles/liter

Normality= 2*molarity

Molality=.15*1100/98*1.1

To calculate the molarity, normality, and molality of the commercially available sample of H2SO4, we first need to gather some information. We have the weight percentage of H2SO4 and the density of the sample. However, we also need the molar mass of H2SO4.

The molar mass of H2SO4 can be calculated by adding up the atomic masses of its constituent elements. H2SO4 contains two hydrogen atoms (H), one sulfur atom (S), and four oxygen atoms (O). Using the periodic table, we find the atomic masses to be:

H: 1.007 g/mol
S: 32.06 g/mol
O: 16.00 g/mol

Calculating the molar mass:
2(1.007 g/mol) + 32.06 g/mol + 4(16.00 g/mol) = 98.09 g/mol

Now that we have the molar mass of H2SO4, let's calculate the desired values:

1. Molarity:
Molarity (M) is defined as the number of moles of solute per liter of solution. In this case, the solute is H2SO4.

Step 1: Calculate the mass of H2SO4 in the given sample.
The sample is 15% H2SO4 by weight, and we are given the density as 1.10 g/mL. So, in 100 g of the solution, there will be 15 g of H2SO4.

Step 2: Convert the mass of H2SO4 to moles.
Moles = mass / molar mass
Moles = 15 g / 98.09 g/mol

Step 3: Convert the volume of the solution to liters.
Since the density is given as 1.10 g/mL, we know that 1 mL of the solution has a mass of 1.10 g. Therefore, 100 g of solution is equal to approximately 90.91 mL (100 g / 1.10 g/mL).

Step 4: Calculate molarity by dividing moles by liters.
Molarity (M) = Moles / Liters
Molarity = (15 g / 98.09 g/mol) / 0.09091 L

Calculate the molarity (M) using the given values.

2. Normality:
Normality (N) is defined as the number of equivalents of solute per liter of solution. Since H2SO4 is a diprotic acid, it can donate two moles of hydrogen ions (H+) per mole of H2SO4.

Step 1: Calculate the moles of H2SO4.
Moles = mass / molar mass
Moles = 15 g / 98.09 g/mol

Step 2: Calculate the number of equivalents of H2SO4.
Equivalents = moles * number of equivalents per mole
Since H2SO4 is a diprotic acid, it donates two moles of H+ per mole of H2SO4.
Equivalents = 2 * (15 g / 98.09 g/mol)

Step 3: Convert the volume of the solution to liters (same as in calculating molarity).

Step 4: Calculate normality by dividing equivalents by liters.
Normality (N) = Equivalents / Liters
Normality = 2 * (15 g / 98.09 g/mol) / 0.09091 L

Calculate the normality (N) using the given values.

3. Molality:
Molality (m) is defined as the number of moles of solute per kilogram of solvent.

Step 1: Calculate the mass of water in the solution.
Since the sample is not pure H2SO4, we need to determine the mass of water by subtracting the mass of H2SO4 from the mass of the solution.
Mass of water = Total mass of the solution - Mass of H2SO4
Mass of water = 100 g - 15 g

Step 2: Convert the mass of water to kilograms.
Mass of water = 85 g / 1000 g/kg

Step 3: Calculate the moles of H2SO4 (same as in calculating molarity).

Step 4: Calculate molality by dividing moles of solute by kilograms of solvent.
Molality (m) = Moles of solute / Kilograms of solvent
Molality = (15 g / 98.09 g/mol) / (85 g / 1000 g/kg)

Calculate the molality (m) using the given values.

By following these steps, you should be able to calculate the molarity, normality, and molality of the commercially available sample of H2SO4.

I believe I see a typo here for molality.

grams H2SO4 = 1100*0.15 = 165 as stated.
mols H2SO4 = 0.15*100/98 as stated.
grams solution = 1100 g as stated
BUT g solvent = 1100-165 = 935g (0.935 kg) so
molality = 0.15*1100/0.935 kg solvent = ?

yes, my eyes are failing.