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What is the mole fraction of sulfuric acid in a solution made by adding 3.4 grams of sulfuric acid to 3,500 mL of water?

 

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To calculate the mole fraction of sulfuric acid in the solution, we need to first determine the amount of sulfuric acid in moles.

The molar mass of sulfuric acid (H2SO4) is:

1 x 2 (hydrogen) = 2
32.07 x 1 (sulfur) = 32.07
16 x 4 (oxygen) = 64
Total = 98.07 g/mol

So, 3.4 grams of sulfuric acid is equal to:

3.4 g / 98.07 g/mol = 0.0347 moles

Next, we need to determine the total moles of solute and solvent in the solution:

• Moles of sulfuric acid = 0.0347 mol
• Moles of water = 3500 mL x 1 L/1000 mL x 18.015 g/mol = 63.261 mol

Therefore, the mole fraction of sulfuric acid in the solution is:

Mole fraction = Moles of sulfuric acid / (Moles of sulfuric acid + Moles of water) = 0.0347 / (0.0347 + 63.261) = 0.00055

So the mole fraction of sulfuric acid is 0.00055.