Final answer:
To make a 0.10 M solution of hydrochloric acid with 1.82 grams of HCl, calculate the moles of HCl and divide by the desired molarity to find the needed volume. You would require a 500 mL volumetric flask.
Step-by-step explanation:
To find out what size volumetric flask is needed to make a 0.10 M solution of hydrochloric acid (HCl) with 1.82 grams of HCl, we first need to calculate the number of moles of HCl. The molar mass of HCl is 36.46 g/mol, so the moles of HCl is calculated as:
moles of HCl = mass (g) / molar mass (g/mol) = 1.82 g / 36.46 g/mol ≈ 0.0499 mol
The formula for molarity (M) is moles of solute (mol) divided by volume of solution (L). Since we want to prepare a 0.10 M HCl solution, we rearrange the formula to solve for the volume:
volume (L) = moles of solute (mol) / molarity (M) = 0.0499 mol / 0.10 M = 0.499 L or 499 mL
Therefore, you would need a 500 mL volumetric flask to prepare a 0.10 M solution of HCl from 1.82 grams of hydrochloric acid. This calculation assumes that the final solution will have a negligible change in volume when the solid is dissolved.