How many miles of HCl will be required to prepare a standard solution of 2mols of HCl?

Answer 1

To calculate the number of milliliters (mL) of hydrochloric acid (HCl) required to prepare a standard solution of 2 mols of HCl, we need to know the concentration of the available HCl solution.

The calculation involves the following steps:

1. Determine the number of moles of HCl desired in the solution.

   Given: 2 mols of HCl

2. Determine the concentration (molarity) of the available HCl solution.

   Let's assume the concentration is 6 M (This is a common concentration for laboratory-grade HCl, but you should use the actual concentration of your solution).

3. Use the molarity equation to calculate the required volume (in liters):

   Molarity (M) = moles of solute / liters of solution

   6 M = 2 mols / liters of solution

   Liters of solution = 2 mols / 6 M

   Liters of solution = 0.333 L

4. Convert the volume from liters to milliliters:

   Volume in mL = Volume in liters × 1000 mL/L

   Volume in mL = 0.333 L × 1000 mL/L

   Volume in mL = 333 mL

Therefore, to prepare a standard solution of 2 mols of HCl using a 6 M HCl solution, you would need approximately 333 mL of the concentrated HCl solution.

Note: The actual volume may vary slightly depending on the precise concentration of the HCl solution you are using and any significant figures involved in the calculation.