Chemistry Fun with Mole Fraction Calculation!
How can we calculate the mole fraction of a solute and a solvent in a solution?
Let's find out how to determine the mole fraction of solute and solvent in a given solution. Let's say we have 583 g of H₂SO₄ in 1.50 kg of water—this acid solution is commonly used in an automobile battery. Can you figure out the mole fraction of H₂SO₄ and water in this solution?
Mole Fraction Calculation:
The mole fraction of H₂SO₄ (solute) and water (solvent) in a solution composed of 583 g of H₂SO₄ and 1.50 kg of water are approximately 0.067 and 0.933, respectively.
To calculate the mole fraction of H₂SO₄ (solute) and water (solvent) in the solution, we first need to determine the number of moles of each substance.
The molecular weight of H₂SO₄ is approximately 98.079 g/mol, so 583 g of H₂SO₄ corresponds to 5.94 moles of H₂SO₄.
The molecular weight of water (H₂O) is approximately 18.015 g/mol. Since we have 1.50 kg (or 1500 g) of water, we therefore have approximately 83.27 moles of water.
The mole fraction of H₂SO₄ can be calculated using the formula: mole fraction = moles of solute / total moles in the solution. Using the numbers obtained earlier, the mole fraction of H₂SO₄ is 5.94 / (5.94 + 83.27) = 0.067.
Similarly, the mole fraction of water is 83.27 / (5.94 + 83.27) = 0.933.
Have fun exploring more about mole fraction calculations and chemistry concepts!