Calculate the concentration of a solution prepared by adding 15.00 mL of
1.92E−3M KMnO4 from a buret into a 50.00 mL volumetric flask, which is then filled to the 50.00 mL graduation mark with distilled water.
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To calculate the concentration of the solution, we can use the formula:
C1V1 = C2V2
Where:
C1 = initial concentration of KMnO4 solution (in M)
V1 = volume of KMnO4 solution added (in L)
C2 = final concentration of the diluted solution (in M)
V2 = final volume of the diluted solution (in L)
Let's calculate the final concentration of the solution by substituting the given values:
C1 = 1.92E-3 M
V1 = 15.00 mL = 15.00/1000 = 0.015 L
C2 = ?
V2 = 50.00 mL = 50.00/1000 = 0.050 L
Using the formula:
C1V1 = C2V2
(1.92E-3 M)(0.015 L) = C2(0.050 L)
0.0000288 M = C2(0.050 L)
C2 = 0.0000288 M / 0.050 L
C2 ≈ 0.000576 M
Therefore, the concentration of the solution prepared by adding 15.00 mL of 1.92E-3 M KMnO4 into a 50.00 mL volumetric flask and filling it to the 50.00 mL mark with distilled water is approximately 0.000576 M.
To calculate the concentration of the solution, you need to determine the final number of moles of KMnO4 in the volumetric flask and then divide it by the total volume of the solution.
Step 1: Calculate the number of moles of KMnO4 added to the flask.
Given that the volume of KMnO4 solution added is 15.00 mL and the concentration is 1.92E-3 M (moles per liter), you can use the formula:
moles = concentration × volume
moles = 1.92E-3 M × 15.00 mL
First, convert the volume to liters:
15.00 mL = 15.00 mL × (1 L / 1000 mL)
15.00 mL = 0.015 L
Substitute the values to calculate the moles:
moles = 1.92E-3 M × 0.015 L
Step 2: Calculate the final volume of the solution in the volumetric flask.
The volumetric flask has an initial volume of 50.00 mL, and 15.00 mL of KMnO4 solution was added, so the final volume is 50.00 mL + 15.00 mL = 65.00 mL.
Convert the final volume to liters:
65.00 mL = 65.00 mL × (1 L / 1000 mL)
65.00 mL = 0.065 L
Step 3: Calculate the final concentration.
Divide the number of moles (obtained in step 1) by the final volume (obtained in step 2):
Concentration (M) = moles / volume
Concentration (M) = (1.92E-3 M × 0.015 L) / 0.065 L
Concentration (M) = (2.88E-5 mol) / 0.065 L
Final concentration = 4.43E-4 M
Therefore, the concentration of the solution prepared by adding 15.00 mL of 1.92E−3M KMnO4 into a 50.00 mL volumetric flask and then filling it to the 50.00 mL graduation mark with distilled water is approximately 4.43E-4 M.