to what volume should you dilute 20 mL of a 10 M H2SO4 solution to obtain a 0.130 M H2SO4 solution?
You want to change the concentration by a factor of .13/10 = .013, so you need to increase the volume by 1/.013 = 76.92
So, 20 * 76.92 = 1538ml
To determine the volume needed to dilute the 20 mL of 10 M H2SO4 solution to obtain a 0.130 M H2SO4 solution, we can use the dilution formula:
C1V1 = C2V2
Where:
C1 = initial concentration of the solution (10 M H2SO4)
V1 = initial volume of the solution (20 mL)
C2 = final concentration of the solution (0.130 M H2SO4)
V2 = final volume of the solution (to be determined)
Rearranging the formula, we have:
V2 = (C1V1) / C2
Substituting the given values, we get:
V2 = (10 M * 20 mL) / 0.130 M
Simplifying the expression, we have:
V2 = 1538.46 mL
Therefore, you should dilute 20 mL of a 10 M H2SO4 solution to a volume of 1538.46 mL (or approximately 1538 mL) to obtain a 0.130 M H2SO4 solution.
To find the volume of the dilution, we can use the equation for dilution:
C₁V₁ = C₂V₂
where C₁ and V₁ are the initial concentration and volume, and C₂ and V₂ are the final concentration and volume.
Let's substitute the given values into the equation:
(10 M)(20 mL) = (0.130 M)(V₂)
Now, we can solve for V₂:
(10 M)(20 mL) / (0.130 M) = V₂
V₂ ≈ 1538.46 mL
Therefore, you should dilute 20 mL of a 10 M H2SO4 solution to approximately 1538.46 mL to obtain a 0.130 M H2SO4 solution.