How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 10.0 L of a solution that has a pH of 2.05?

Verified step by step guidance

1. Calculate the concentration of hydrogen ions \([H^+]\) in the target solution using the pH value. Use the formula \([H^+] = 10^{-\text{pH}}\).
2. Determine the molarity of the target solution. Since \([H^+]\) is equal to the molarity of HCl in the solution, use the concentration from step 1.
3. Calculate the moles of HCl needed in the target solution by multiplying the molarity from step 2 by the volume of the solution in liters (10.0 L).
4. Determine the mass of HCl required using the moles calculated in step 3 and the molar mass of HCl (36.46 g/mol).
5. Calculate the volume of the concentrated HCl solution needed. Use the mass of HCl from step 4, the percentage by mass (36.0%), and the density (1.18 g/mL) to find the volume in milliliters.