How many milliliters of 3.0 M hydrochloric acid are i required to prepare 500 milliliter of 1.0 M Hydrochloric solution

The general dilution equation is: C1V1 = C2V2, where C = concentration and V = volume 3.0 M x V1 = 1.0 M x 500 mL V1 = 1.0 M x 500 mL / 3.0 M = 167 mL Add 167 mL of 3.0 M HCl to enough water to make 500 mL of solution

To find the number of milliliters of 3.0 M hydrochloric acid required to prepare 500 milliliters of 1.0 M hydrochloric solution, we can use the equation:

(C1)(V1) = (C2)(V2)

where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume.

In this case, C1 = 3.0 M, V1 is the unknown volume we want to find, C2 = 1.0 M, and V2 = 500 mL.

Rearranging the equation, we have:

V1 = (C2)(V2) / C1

Now, plugging in the values:

V1 = (1.0 M)(500 mL) / 3.0 M

V1 = 500 mL / 3

V1 ≈ 166.67 mL

Therefore, we would need approximately 166.67 milliliters of 3.0 M hydrochloric acid to prepare 500 milliliters of 1.0 M hydrochloric solution.