Final answer:
To prepare a 2.00 L solution of 0.15 M sulfuric acid from 18 M concentrated sulfuric acid, 16.7 mL of the concentrated acid must be diluted to the final volume.
Step-by-step explanation:
To prepare 2.00 L of a 0.15 M sulfuric acid (H2SO4) solution from concentrated (18 M) sulfuric acid, we first calculate the number of moles of H2SO4 required using the equation:
Molarity (M) = moles of solute / volume of solution in liters
Therefore, moles of H2SO4 = Molarity × Volume = 0.15 M × 2.00 L = 0.30 moles.
Next, we use the molarity of the concentrated sulfuric acid to find the required volume to obtain 0.30 moles:
Volume of concentrated H2SO4 = moles of H2SO4 / Molarity = 0.30 moles / 18 M = 0.0167 L, which is 16.7 mL.
So, to prepare the desired solution, 16.7 mL of concentrated 18 M sulfuric acid should be carefully diluted with water to a final volume of 2.00 L.