how to prepare 0.100M HCL solution when laboratory grade concentrated by hydrochloric acid has concentration of 37%.what volume of acid is necessary to prepare 500mL of 0.100M of HCL

To prepare a 0.100M HCl solution, you need to calculate the volume of concentrated hydrochloric acid (HCl) required by using the molarity, volume, and concentration relationship. Here are the steps to determine the necessary volume:

Step 1: Determine the number of moles of HCl required.
- Molarity of the desired HCl solution = 0.100M
- Volume of the desired HCl solution = 500 mL = 0.500 L
- Moles of HCl = Molarity × Volume
= 0.100 mol/L × 0.500 L
= 0.050 mol

Step 2: Convert the number of moles of HCl to the volume of concentrated HCl.

To calculate the required volume, you need the concentration of the concentrated HCl. In this case, it is given as 37%.

- Concentration of the concentrated HCl solution = 37%
- Concentration is written as grams of solute per 100 mL of solution. Therefore, the concentration needs to be converted to moles per liter.

- Mass of the concentrated HCl solution = 37 g/100 mL = 37 g/0.100 L (since 1 L = 1000 mL)
- Moles of the concentrated HCl = mass/concentration

Moles of concentrated HCl = 37 g/0.100 L ÷ 36.4611 g/mol (molecular weight of HCl)

Step 3: Calculate the volume of concentrated HCl.
- Moles of HCl required = 0.050 mol (from Step 1)
- Moles of concentrated HCl available = 37 g/0.100 L ÷ 36.4611 g/mol (from Step 2)

Since moles = volume/concentration, we can rearrange the equation to solve for the volume.

Volume of concentrated HCl required = Moles of HCl required ÷ Moles of concentrated HCl available
= 0.050 mol ÷ (37 g/0.100 L ÷ 36.4611 g/mol)
= 50 mL

Therefore, you would need 50 mL of concentrated HCl to prepare a 0.100M HCl solution with a total volume of 500 mL.