Final answer:
To make 250 ml of a 1.22 M sulfuric acid solution, one would need 29.92 grams of sulfuric acid, calculated by multiplying the molarity by the volume in liters and the molar mass of sulfuric acid.
Step-by-step explanation:
To determine how many grams of sulfuric acid (H2SO4) are needed to make 250 ml of a 1.22 M solution, we follow these steps:
Calculate the number of moles of H2SO4 using the volume of the solution and its molarity: Moles = Molarity × Volume (in liters).
Convert the volume from milliliters to liters by dividing by 1000.
Calculate the mass of sulphuric acid using its molar mass and the number of moles calculated in the first step: Mass = Moles × Molar mass.
Use the molar mass of H2SO4, which is 98.079 g/mol.
For a 1.22 M solution of H2SO4 in 250 ml:
Convert 250 ml to liters: 0.250 L.
Calculate the number of moles: 1.22 mol/L × 0.250 L = 0.305 moles.
Calculate the mass: 0.305 moles × 98.079 g/mol = 29.92 grams.
Therefore, you need 29.92 grams of sulfuric acid to make 250 ml of a 1.22 M solution.