Question

Determine the volume of additional pure water required to convert 0.10 L of 0.0100 M KMnO4 solution into its 0.00500 M solution.

Answer 1

To convert the given solution of KMnO4 into a desired concentration, we can use the concept of dilution. By applying the dilution formula, we can determine the volume of additional water needed. In this case, an additional 0.2 L of pure water is required to convert the solution.

Step-by-step explanation:

To determine the volume of additional pure water required to convert 0.10 L of 0.0100 M KMnO4 solution into its 0.00500 M solution, we can use the concept of dilution. The formula for dilution is M1V1 = M2V2, where M1 and V1 are the initial concentration and volume, and M2 and V2 are the final concentration and volume respectively. In this case, we are given the initial concentration and volume, and we need to find the final volume. Let's plug in the values:

M1 = 0.0100 M, V1 = 0.10 L, M2 = 0.00500 M, and solve for V2:

1. M1V1 = M2V2
2. (0.0100 M)(0.10 L) = (0.00500 M)(V2)
3. 0.001 M*L = 0.00500 M * V2
4. V2 = 0.001 M*L / 0.00500 M
5. V2 = 0.2 L

Therefore, an additional 0.2 L of pure water is required to convert 0.10 L of 0.0100 M KMnO4 solution into its 0.00500 M solution.