Potassium permangenat reacts with sodium oxalate to form carbon dioxide and Mn2+.determine the consentration of a permangenate solution.since the reaction runs in acidic conditions, 25ml of 2 M sulfuric acid was added to 20.00ml of the unknown permangenate solution. It was then titrated with 21.15ml of a 0.111M oxalate solution. what strength was the permangenate solution?
2MnO4^- + 5C2O4^2- ==> 10CO2 + 2Mn^2+
(Note: that doesn't balance all of the equation but the H2SO4, K^+, etc are just spectator ions.)
mols C2O4^2- = M x L = 0.111 x 0.02115=?
Using the coefficients in the balanced equation, convert mols C2O4^2- to mols MnO4^-. That will be ? mols C2O4^2- x (2 mols MnO4^-/5 mols C2O4^2-) = ?
Then M MnO4^- = mols MnO4^-/L MnO4^-. You have mols and L, solve for M.
To determine the concentration of the permanganate solution, we can use the concept of stoichiometry.
Let's break down the given information:
1. The reaction between potassium permanganate (KMnO4) and sodium oxalate (Na2C2O4) is as follows:
2KMnO4 + 3Na2C2O4 + 4H2SO4 -> K2SO4 + 2MnSO4 + 3Na2SO4 + 8CO2 + 4H2O
From the balanced reaction, we know that for every 2 moles of KMnO4, 3 moles of Na2C2O4 react.
2. The reaction runs in acidic conditions. Therefore, 25 ml of 2 M sulfuric acid (H2SO4) was added to 20.00 ml of the unknown permanganate solution. The purpose of adding sulfuric acid is to create an acidic environment required for the reaction to occur.
3. The permanganate solution is being titrated with a 0.111 M oxalate solution (Na2C2O4).
4. The volume of the oxalate solution used in titration is 21.15 ml.
Now, let's calculate the concentration of the permanganate solution (KMnO4).
First, we need to calculate the moles of oxalate used in the titration:
Moles of oxalate = Molarity (oxalate) x Volume (oxalate)
= 0.111 mol/L x 0.02115 L
= 0.00234 mol
From the balanced reaction, we know that 3 moles of oxalate react with 2 moles of permanganate.
Therefore, the moles of permanganate (KMnO4) used in the reaction will be:
Moles of permanganate = (3/2) x Moles of oxalate
= (3/2) x 0.00234 mol
= 0.00351 mol
As we know that the total final volume of the permanganate solution is 20 ml + 25 ml = 45 ml,
we can calculate the concentration of the permanganate solution (KMnO4).
Concentration (KMnO4) = Moles of permanganate / Volume (MnO4)
= 0.00351 mol / 0.045 L
= 0.078 M
Therefore, the strength of the permanganate solution is 0.078 M (molar concentration).