solution of hydrogen peroxide, H2O2 , is titrated with potassium permanganate, KMnO4 , according to the following equation:

Question

solution of hydrogen peroxide, H2O2 , is titrated with potassium permanganate, KMnO4 , according to the following equation:

5 H2O2 + 2 KMnO4+ 3H2SO4 -> 5O2 + 2 MnSO4 +8H2O + K2SO4

It requires 46.9mL of 0.145 mol/L KMnO4 to titrate 50.0 mL of the solution of H2O2 .

What is the moles per litre concentration of H2O2 in the solution?

I cant even figure out the first step in converting cause don't you need to convert it to moles/liters

Answer 1

Yes, you are correct. To find the moles per litre concentration of H2O2 in the solution, you first need to convert the volume and concentration provided for KMnO4 to moles.

First, let's convert the volume of KMnO4 solution given to moles:
Volume of KMnO4 = 46.9 mL
Concentration of KMnO4 = 0.145 mol/L

To convert mL to L, divide the volume by 1000:
46.9 mL = 46.9/1000 = 0.0469 L

Now, we can use the equation C = n/V, where C is the concentration in mol/L, n is the number of moles, and V is the volume in liters.

So, the number of moles of KMnO4 can be calculated as follows:
n(KMnO4) = C(KMnO4) * V(KMnO4) = 0.145 mol/L * 0.0469 L = 0.006813 moles of KMnO4

Now, let's find the number of moles of H2O2 using the stoichiometry of the balanced equation.

From the balanced equation, we can see that the molar ratio between KMnO4 and H2O2 is 2:5.
That means, for every 2 moles of KMnO4, there are 5 moles of H2O2.

Using the molar ratio, we can determine the moles of H2O2:
n(H2O2) = (n(KMnO4) * 5) / 2 = (0.006813 mol * 5) / 2 = 0.01703325 moles of H2O2

Next, we need to find the volume of H2O2 solution used in the titration.

Volume of H2O2 solution = 50.0 mL

Again, convert mL to L:
50.0 mL = 50.0/1000 = 0.0500 L

Finally, we can calculate the concentration of H2O2 in moles per litre (mol/L):
C(H2O2) = n(H2O2) / V(H2O2) = 0.01703325 moles / 0.0500 L = 0.340665 mol/L

Therefore, the moles per litre concentration of H2O2 in the solution is 0.340665 mol/L.

Answer 2

To determine the moles per liter concentration of H2O2 in the solution, you need to use the information provided in the question.

First, calculate the number of moles of KMnO4 used in the titration:
Moles of KMnO4 = (Volume of KMnO4 used in titration) x (Concentration of KMnO4)
= (46.9 mL) x (0.145 mol/L)
= 6.7985 mmol

Next, determine the stoichiometric ratio between KMnO4 and H2O2 from the balanced chemical equation:
2 moles of KMnO4 : 5 moles of H2O2
So, for every 2 moles of KMnO4 used, 5 moles of H2O2 will react.

Now, convert the moles of KMnO4 used to moles of H2O2:
Moles of H2O2 = (Moles of KMnO4) x (5 moles of H2O2 / 2 moles of KMnO4)
= (6.7985 mmol) x (5/2)
= 16.9975 mmol

Finally, convert the moles of H2O2 to the moles per liter concentration (mol/L):
Concentration of H2O2 = (Moles of H2O2) / (Volume of H2O2 used in titration)
= (16.9975 mmol) / (50.0 mL)
= 0.33995 mol/L

Therefore, the moles per liter concentration of H2O2 in the solution is approximately 0.33995 mol/L.

Answer 3

I wrote specific instructions for you to solve this problem several problems below. Follow them step by step. If you get stuck, shoe your work ANB tell me what you don't understand about the next step. What's the first step? Determine mols KMnO4 and mols KMnO4 = M x L. The molarity AND volume of KMnO4 are given.

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