What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?
Find:
V1 : initial volume
Given:
C1=2.5M : initial concentration
C2=0.50M : final concentration
V2=100.0mL : final volume
Using:
V1 = V2 * C2 / C1
56
To solve this problem, we need to use the formula for dilution:
M₁V₁ = M₂V₂
Where:
M₁ = initial molarity of the stock solution
V₁ = initial volume of the stock solution
M₂ = final molarity of the diluted solution
V₂ = final volume of the diluted solution
In this case:
M₁ = 2.5 M
V₁ = ?
M₂ = 0.50 M
V₂ = 100.0 mL
Rearranging the formula to solve for V₁, we have:
V₁ = (M₂ * V₂) / M₁
Substituting the values:
V₁ = (0.50 M * 100.0 mL) / 2.5 M
Now we can calculate:
V₁ = (0.50 * 100.0) / 2.5
V₁ = 20.0 mL
Therefore, you would need to take 20.0 milliliters of the 2.5 M acetic acid stock solution and dilute it to 100.0 milliliters to prepare a 0.50 M acetic acid solution.