Question

Problem 6.23

Sulfuric acid is normally purchased at a concentration of 18.6M.

Part A

How would you prepare 250.0mL of 0.650M aqueous H2SO4? (Remember to add the acid to water rather than water to the acid.)

How would you prepare  of  aqueous ? (Remember to add the acid to water rather than water to the acid.)

Mi×Vi=Mf×Vf; Vi=Mf×Vf/Mi=0.650M×250.0mL/18.6M=8.74mL
Dilute 8.74mL of 18.6M H2SO4 with enough water to make 250.0mL of solution. The resulting solution will be 0.650M H2SO4

Mi/Vi=Mf/Vf; Vi=Mi×Vf/Mf=18.6M×250.0mL/0.650M=7150mL
Dilute 7150mL of 18.6M H2SO4 with enough water to make 250.0mL of solution. The resulting solution will be 0.650M H2SO4

Vi=Mi/Mf=18.6M/0.650M=28.6mL
Dilute 28.6mL of 18.6M H2SO4 with enough water to make 250.0mL of solution. The resulting solution will be 0.650M H2SO4

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Answer 1

use dilution formula

M1*V1 = M2*V2

Here:

M1 is molarity of solution before dilution

M2 is molarity of solution after dilution

V1 is volume of solution before dilution

V2 is volume of solution after dilution

we have:

M1 = 18.6 M

M2 = 0.65 M

V2 = 250.0 mL

we have below equation to be used:

M1*V1 = M2*V2

V1 = (M2 * V2) / M1

V1 = (0.65*250)/18.6

V1 = 8.74 mL

So we should take 8.74 mL of 18.6 M solution with enough water.

Answer: option 1