Calculate the MnO4- concentration of the diluted sample when the sample is prepared in the following manner: Add 2 drops oxalic acid, 4 drops permanganate and 8 drops water. The original permanganate is 0.25M.
I don't understand how to do this, any help would be appreciated.
The reaction is...
2MnO4−+5H2C2O4+6H+>>2Mn2++10CO2
+8H2O.
Normally, a drop or two of sulfuric acid is added to provide the H+ ion, however, if you have excess oxalic acid, it should provide enough.
So you had 4 drops , diluted with 10 drops, to a new volume of 14 drops. So Molarity before the reaction will be .25*(4/14). Now as the reaction goes to completion, no permanganate ion remains.
yes, the 2 drops of oxalic acid, and 8 drops of water are mostly diluting water.
To calculate the MnO4- concentration in the diluted sample, we need to use the concept of dilution. Dilution is a technique used to decrease the concentration of a solute by adding more solvent.
In this case, we are given that the original permanganate (MnO4-) concentration is 0.25M. The diluted sample is prepared by adding 2 drops of oxalic acid, 4 drops of permanganate, and 8 drops of water.
To calculate the concentration of MnO4- in the diluted sample, we can use the equation:
(C1)(V1) = (C2)(V2)
Where:
C1 = Initial concentration
V1 = Initial volume
C2 = Final concentration
V2 = Final volume
Now let's plug in the values we have:
Initial concentration (C1) = 0.25M
Initial volume (V1) = 4 drops (since we are adding 4 drops of permanganate)
Final volume (V2) = 2 drops (since we are adding 2 drops of oxalic acid)
We need to find the final concentration (C2) of the MnO4- in the diluted sample.
Using the equation (C1)(V1) = (C2)(V2), we can rearrange the equation to solve for C2:
C2 = (C1)(V1) / V2
Substituting the given values:
C2 = (0.25M)(4 drops) / 2 drops
C2 = 1M
Therefore, the MnO4- concentration in the diluted sample is 1M.
To find the concentration of the MnO4- in the diluted sample, we can use the concept of dilution.
First, note that the original permanganate concentration is 0.25M.
Let's assume that the volume of each drop is negligible. This means that the number of drops does not affect the final concentration.
In this case, the diluted sample is prepared by adding 2 drops of oxalic acid, 4 drops of permanganate, and 8 drops of water.
To determine the final concentration, we need to account for the dilution factor. The dilution factor is calculated by dividing the final volume by the initial volume.
Let's assume that each drop has a volume of 1 mL for simplicity. So, the initial volume is 4 mL (4 drops of permanganate), and the final volume is 14 mL (2 drops oxalic acid + 4 drops permanganate + 8 drops water).
Now we can calculate the dilution factor:
Dilution factor = final volume / initial volume = 14 mL / 4 mL = 3.5
Since the original permanganate concentration is given in moles per liter (M), we need to convert the dilution factor to liters:
Dilution factor = 3.5 L
Now, to find the final MnO4- concentration, we can use the formula:
Final concentration = initial concentration / dilution factor
Final concentration = 0.25 M / 3.5 = 0.0714 M (rounded to four decimal places)
Therefore, the MnO4- concentration of the diluted sample is approximately 0.0714 M.