High School

1.00 L of 6.00 M HCl is used to prepare exactly 100 mL of 1.00 M HCl. How many mL of the 6.00 M HCl must be diluted with water to prepare the 1.00 M HCl solution?

Answer :

Final answer:

To prepare a 1.00M HCl solution of volume 100mL from a 6.00M HCl solution, you need to take 16.7mL of the 6.00 M HCl solution and dilute it to a total volume of 100mL.

Explanation:

The question is about preparing a 1.00M HCl solution by diluting a 6.00M HCl solution. Using the concept of molarity, M1V1 = M2V2, where M1 is the initial molarity (6.00M), V1 is the volume to be determined, M2 will be the final molarity (1.00M), and V2 is the final volume (100mL or 0.100L).

Calculate V1 by manipulating the formula, V1 = (M2*V2) / M1 = (1.00M * 0.100L) / 6.00M = 0.0167L or 16.7mL. To prepare a 1.00M solution of 100mL, you will need to take 16.7mL of the 6.00M HCl solution and dilute it to a total volume of 100mL with water.

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