Find the a) % solution, b) molality and c) mole fraction of the acid 16.0 M H2SO4 d = 1.634 g/ml for the solution
density = 1.634 g/mL.
mass of 1000 mL = 1.634 g/mL x 1000 mL = 1634 grams.
M = mols/L = 16.0 mols/liter of solution; therefore, we have 16.0 mols in 1634 g solution.
16.0 mols H2SO4 = 16.0 mols x 98 g/mol = 1568 g H2SO4.
%H2SO4 = (1568 g H2SO4/1634 g soln)*100 = xx % H2SO4.
mole fraction H2SO4= mols H2SO4/(mols H2SO4 + mols H2O).
You have mols H2SO4 from above. Grams H2O = 1634-1568 = yy g H2O and that divided by 18 = mols H2O.
molality = mols/kg solvent. You have mols H2SO4 and you have g H2O (from the mole fraction calculation). Change g H2O to kg and you have it.
Post your work if you get stuck. Check my thinking.
To find the % solution, molality, and mole fraction of the acid solution, we need to use the given concentration of H2SO4 solution and its density.
a) % Solution:
The % solution can be calculated by dividing the mass of the solute (H2SO4) by the total mass of the solution and then multiplying by 100.
First, let's calculate the mass of H2SO4 in 1 liter of the solution:
Density (d) = 1.634 g/ml
Since the density is given in grams per milliliter, we can assume that 1 liter of the solution has a mass of 1634 grams (1.634 g/ml x 1000 ml).
The concentration of H2SO4 is given as 16.0 M, which means there are 16.0 moles of H2SO4 in 1 liter of the solution.
To calculate the mass of H2SO4, we need to use its molar mass. The molar mass of H2SO4 is:
(2 * Atomic mass of H) + Atomic mass of S + (4 * Atomic mass of O)
= (2 * 1.01 g/mol) + 32.07 g/mol + (4 * 16.00 g/mol)
= 98.09 g/mol
Now, let's find the mass of H2SO4 in 1 liter of the solution:
Mass of H2SO4 = Concentration (M) x Volume (L) x Molar mass (g/mol)
= 16.0 mol/L x 1 L x 98.09 g/mol
= 1569.44 g
Finally, let's calculate the % solution:
% Solution = (Mass of H2SO4 / Total mass of the solution) x 100
= (1569.44 g / 1634 g) x 100
= 95.95%
Therefore, the % solution of the H2SO4 solution is approximately 95.95%.
b) Molality:
Molality is defined as the number of moles of solute (H2SO4) per kilogram of solvent (water).
The molar mass of H2SO4 is 98.09 g/mol (as calculated in part a).
We know that there are 16.0 moles of H2SO4 in 1 liter of the solution.
The mass of water (solvent) in the solution can be calculated using the density:
Mass of 1 liter of the solution = Density (g/ml) x Volume (ml)
= 1.634 g/ml x 1000 ml
= 1634 g
Now, let's calculate the molality:
Molality = (Number of moles of H2SO4 / Mass of water in kg)
= (16.0 mol / 1.634 kg)
= 9.8 mol/kg (rounded to one decimal place)
Therefore, the molality (m) of the H2SO4 solution is approximately 9.8 mol/kg.
c) Mole Fraction:
The mole fraction (X) of a component in a solution is defined as the ratio of the moles of that component to the total moles of all components in the solution.
To calculate the mole fraction of H2SO4, we need to know the number of moles of other components in the solution (if any).
If the solution only contains H2SO4 and water, then the mole fraction of H2SO4 is simply the ratio of its moles to the total moles:
Mole fraction of H2SO4 = Moles of H2SO4 / Total moles
Since the concentration of H2SO4 is 16.0 M, there are 16.0 moles of H2SO4 in 1 liter of the solution.
The mass of water in the solution can be calculated as mentioned earlier:
Mass of water = 1634 g
To find the moles of water, we need to use its molar mass. The molar mass of water (H2O) is 18.02 g/mol.
Moles of water = Mass of water / Molar mass of water
= 1634 g / 18.02 g/mol
= 90.6 mol
Now let's calculate the mole fraction of H2SO4:
Mole fraction of H2SO4 = 16.0 mol / (16.0 mol + 90.6 mol)
= 16.0 mol / 106.6 mol
≈ 0.150 (rounded to three decimal places)
Therefore, the mole fraction (X) of the acid H2SO4 in the solution is approximately 0.150.