A stock solution of 0.0100 M KMnO4
is diluted by taking 15.5 mL of it
and diluting it to 100.0 mL. From this diluted solution, 5.00 mL is taken
out and diluted to 100.0 mL. What is the concentration of the solution
obtained in the end
0.01 x (15.5/100) x (5/100) = ?
To determine the concentration of the solution obtained in the end, we need to use the concept of dilution. Dilution is the process of adding solvent (usually water) to a stock solution to decrease its concentration.
Let's break down the dilution process step by step:
1. Initial concentration: The initial concentration of the stock solution is given as 0.0100 M KMnO4.
2. First dilution: To dilute the stock solution, 15.5 mL of it is taken and diluted to a final volume of 100.0 mL. We can use the dilution formula C1V1 = C2V2 to calculate the new concentration.
C1 = Initial concentration = 0.0100 M
V1 = Initial volume = 15.5 mL
V2 = Final volume = 100.0 mL
C2 = ?
Applying the dilution formula:
(0.0100 M)(15.5 mL) = C2(100.0 mL)
C2 = (0.0100 M)(15.5 mL) / (100.0 mL)
= 0.00155 M
The concentration of the solution after the first dilution is 0.00155 M KMnO4.
3. Second dilution: From the diluted solution obtained above, 5.00 mL is taken and diluted to a final volume of 100.0 mL. We can use the same dilution formula to calculate the final concentration once again.
C1 = Previous concentration = 0.00155 M
V1 = Previous volume = 5.00 mL
V2 = Final volume = 100.0 mL
C2 = ?
Applying the dilution formula:
(0.00155 M)(5.00 mL) = C2(100.0 mL)
C2 = (0.00155 M)(5.00 mL) / (100.0 mL)
= 0.0000775 M
The concentration of the solution obtained in the end after the second dilution is 0.0000775 M KMnO4.