How much water must be added to 500.0 mL of a 3.00 M HCl solution to obtain a solution that is 2.00 M?

Question

Quizplus · Accepted Answer

To obtain a solution that is 2.00 M, the number of moles of HCl must remain the same. The number of moles of HCl in 500.0 mL of a 3.00 M HCl solution is:```moles of HCl = (500.0 mL) × (3.00 mol/L) = 1500 mmol```To obtain a 2.00 M solution, the volume of the solution must be increased to:```volume of solution = (1500 mmol) / (2.00 mol/L) = 750 mL```Therefore, the amount of water that must be added is:```volume of water = (750 mL) - (500.0 mL) = 250 mL```Converting to liters, we get:```volume of water = 250 mL × (1 L / 1000 mL) = 0.250 L```Therefore, the correct answer is D) 2.50 × 10² mL.

How Much Water Must Be Added to 500