To make 500 ml of 1.0 M H2SO4 solution, we need to calculate the amount of H2SO4 needed in moles, and then determine the volume of the 12 M stock solution required to provide that amount of H2SO4.
The amount of H2SO4 needed in moles can be calculated using the following equation:
moles of solute = Molarity × Volume of solution (in liters)
Since we want to make 500 ml (0.5 L) of 1.0 M H2SO4 solution, we can rearrange the above equation to solve for moles of solute:
moles of solute = Molarity × Volume of solution (in liters)
moles of solute = 1.0 M × 0.5 L
moles of solute = 0.5 moles
So we need 0.5 moles of H2SO4 for this solution.
Now we can use the molarity and volume of the stock solution to calculate the volume of the stock solution needed:
Molarity of stock solution × Volume of stock solution = moles of solute
Rearranging the equation, we get:
Volume of stock solution = moles of solute / Molarity of stock solution
Substituting the values we have:
Volume of stock solution = 0.5 moles / 12 M
Volume of stock solution = 0.0417 L or 41.7 mL (rounded to the nearest tenth)
Therefore, we need 41.7 mL of the 12 M H2SO4 stock solution to make 500 mL of 1.0 M H2SO4 solution.