The Volume of a Diluted KNO3 Solution
A chemist dilutes a 1.0 mL sample of 2.0 M KNO3 by adding water to it. If the concentration of the solution that is obtained is 0.0080 M, what is its volume? Use the equation:
(initial concentration) x (initial volume) = (final concentration) x (final volume)
So:
(2 M) x (1ml) = (.008 M) x (X ml)
X = 250 ml
Answer: The volume of the diluted solution is 250 mL.
Explanation: To calculate the molarity of the diluted solution, we use the equation:
M₁V₁ = M₂V₂
where, M₁ and V₁ are the molarity and volume of the concentrated KNO3 solution and M₂ and V₂ are the molarity and volume of the diluted KNO3 solution.
We are given:
M₁ = 2M
V₁ = 1mL
M₂ = 0.008M
V₂ = ?mL
Putting values in the above equation, we get:
2 x 1 = 0.008 x V₂
V₂ = 250mL
Hence, the volume of the diluted solution is 250 mL.
What is the equation used to calculate the volume of a diluted solution in this scenario?
The equation used to calculate the volume of the diluted solution in this scenario is (initial concentration) x (initial volume) = (final concentration) x (final volume).