![Calculate the target hydrogen ion concentration ([H^+]) from the desired pH.](/_next/image?url=https%3A%2F%2Fohijasnjvprzodcmxltt.supabase.co%2Fstorage%2Fv1%2Fobject%2Fpublic%2Fwhatsapp-images%2F1779227732732-0fff9f7fee0bf514.png&w=3840&q=75)
This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
You're on a roll — let's tackle this dilution problem. Step 1: Calculate the target hydrogen ion concentration ([H^+]) from the desired pH. Since HCl is a strong acid, it dissociates completely, so [H^+] = [HCl]. [H^+] = 10^-pH [H^+] = 10^-2.10 [H^+] = 7.943 × 10^-3 M Therefore, the target concentration of HCl in the final solution is 7.943 × 10^-3 M. Step 2: Calculate the total moles of HCl needed for the final solution. The final volume is 12.5 L. Moles of HCl = Concentration × Volume Moles of HCl = (7.943 × 10^-3 mol/L) × (12.5 L) Moles of HCl = 0.0992875 mol Step 3: Calculate the molarity of the concentrated HCl solution. The concentrated HCl is 36.0% HCl by mass and has a density of 1.18 g/mL. Assume we have 100 g of the concentrated solution. Mass of HCl in 100 g solution = 36.0 g Volume of 100 g solution = MassDensity = 100 g1.18 g/mL = 84.746 mL = 0.084746 L Molar mass of HCl = 1.008 g/mol (H) + 35.45 g/mol (Cl) = 36.458 g/mol Moles of HCl in 36.0 g = 36.0 g36.458 g/mol = 0.9874 mol Molarity of concentrated HCl = Moles of HClVolume of solution (L) Molarity of concentrated HCl = 0.9874 mol0.084746 L = 11.651 M Step 4: Calculate the volume of concentrated HCl required. We need 0.0992875 mol of HCl (from Step 2) and the concentrated solution is 11.651 M (from Step 3). Volume of concentrated HCl = Moles of HClMolarity of concentrated HCl Volume of concentrated HCl = 0.0992875 mol11.651 mol/L Volume of concentrated HCl = 0.008521 L Convert the volume to milliliters: Volume of concentrated HCl = 0.008521 L × 1000 mL/L = 8.521 mL Rounding to three significant figures (due to 36.0% and pH 2.10): The volume of concentrated HCl required is 8.52 mL. What's next?