Titration of 50.00 mL of 0.0521 M sodium oxalate, Na2C2O4, required 38.71 mL of a potassium permanganate solution:
5 C2O42- + 2MnO4- + 16H+ = 2Mn2+ + 10 CO2 + 8H2O
Calculate the molarity of the potassium permanganate solution.
Well, it seems like we're doing some chemistry here! Let's calculate the molarity of the potassium permanganate solution.
First, let's write down the balanced chemical equation for the reaction:
5 C2O42- + 2 MnO4- + 16 H+ → 2 Mn2+ + 10 CO2 + 8 H2O
From the equation, we can see that the mole ratio between C2O42- and MnO4- is 5:2.
Let's calculate the number of moles of sodium oxalate, Na2C2O4:
Moles of Na2C2O4 = volume (L) × concentration (M)
Moles of Na2C2O4 = 0.050 L × 0.0521 M
Moles of Na2C2O4 = 0.002605 mol
Since the mole ratio between C2O42- and MnO4- is 5:2, the number of moles of MnO4- can be calculated as:
Moles of MnO4- = (5/2) × moles of Na2C2O4
Moles of MnO4- = (5/2) × 0.002605 mol
Moles of MnO4- = 0.0065125 mol
Now, we need to find the molarity of the potassium permanganate solution. To do that, we divide the number of moles of MnO4- by the volume in liters:
Molarity = moles/volume
Molarity = 0.0065125 mol / 0.03871 L
Molarity ≈ 0.168 M
So, the molarity of the potassium permanganate solution is approximately 0.168 M.
I hope my answer didn't leave you feeling oxidized!
To calculate the molarity of the potassium permanganate (KMnO4) solution, we can use the balanced chemical equation and the stoichiometry of the reaction.
From the balanced equation:
5 C2O42- + 2 MnO4- + 16 H+ -> 2 Mn2+ + 10 CO2 + 8 H2O
The stoichiometric ratio between sodium oxalate (Na2C2O4) and potassium permanganate (KMnO4) is 5:2. This means that 5 moles of sodium oxalate react with 2 moles of potassium permanganate.
Given:
Volume of KMnO4 solution = 38.71 mL
Molarity of Na2C2O4 solution = 0.0521 M
Volume of Na2C2O4 solution = 50.00 mL
First, let's calculate the number of moles of Na2C2O4 used in the titration:
moles of Na2C2O4 = Molarity * Volume
= 0.0521 M * (50.00 mL / 1000 mL/ L)
= 0.002605 mol
Using the stoichiometry of the reaction, we can determine the number of moles of KMnO4 used in the titration:
moles of KMnO4 = (2/5) * moles of Na2C2O4 (using the stoichiometric ratio)
= (2/5) * 0.002605 mol
= 0.001042 mol
Next, let's calculate the molarity of the KMnO4 solution:
Molarity = moles / Volume
= 0.001042 mol / (38.71 mL / 1000 mL/L)
= 0.0269 M
Therefore, the molarity of the potassium permanganate solution is approximately 0.0269 M.
To calculate the molarity of the potassium permanganate (KMnO4) solution, we can use the concept of stoichiometry and the balanced chemical equation provided.
First, let's start by identifying the stoichiometric ratio between the reactants based on the balanced equation:
5 C2O42- + 2MnO4- + 16H+ = 2Mn2+ + 10 CO2 + 8H2O
From the equation, we can see that the stoichiometric ratio between C2O42- (sodium oxalate) and MnO4- (potassium permanganate) is 5:2.
Next, let's convert the volume of the potassium permanganate solution used in the titration to moles using its molar ratio:
38.71 mL of KMnO4 * (1 L / 1000 mL) * (0.0521 mol/L KMnO4) = 0.02016 mol KMnO4
Now, based on the stoichiometric ratio, we can determine the number of moles of C2O42- reacted with the KMnO4:
0.02016 mol KMnO4 * (5 mol C2O42- / 2 mol KMnO4) = 0.0504 mol C2O42-
Finally, we can calculate the molarity (M) of the KMnO4 solution by dividing the moles of KMnO4 by the volume of the C2O42- solution used in the titration:
Molarity of KMnO4 solution = (0.02016 mol KMnO4) / (50.00 mL of C2O42- * (1 L / 1000 mL)) = 0.4032 M
Therefore, the molarity of the potassium permanganate solution is 0.4032 M.
mols Na2C2O4 = M x L = ?
Use the coefficients in the balanced equation to convert mols Na2C2O4 to mols KMnO4.
Then M KMnO4 = mols KMnO4/L KMnO4