Calculate the amount of h2so4 required for preparing 500ml of 2MH2so4 solution.
well, that would be 1 mole, right?
To calculate the amount of H2SO4 required for preparing a 2M H2SO4 solution, you need to know the molar mass of H2SO4 and the desired volume of the solution.
Step 1: Find the molar mass of H2SO4:
The molar mass of hydrogen (H) is approximately 1 g/mol, sulfur (S) is approximately 32 g/mol, and oxygen (O) is approximately 16 g/mol.
So, the molar mass of H2SO4 = (2 x 1) + 32 + (4 x 16) = 98 g/mol.
Step 2: Convert the desired volume of the solution to liters:
Given that you want to prepare 500 mL of the solution, you need to convert it to liters by dividing it by 1000:
500 mL ÷ 1000 = 0.5 L.
Step 3: Calculate the number of moles of H2SO4 required:
Using the formula: moles = Molarity x Volume (in liters), we can substitute the values:
moles = 2 M x 0.5 L = 1 mole.
Step 4: Calculate the amount of H2SO4 in grams:
To convert moles to grams, you multiply the number of moles by the molar mass of H2SO4:
grams = moles x molar mass = 1 mole x 98 g/mol = 98 grams.
Therefore, you would need 98 grams of H2SO4 to prepare 500 mL of a 2M H2SO4 solution.