A 3.4g sample of h2o2 solution containing x% H2O2 by mass requires x ml of a KMnO4 solution for complete oxidation under acidic condition. the molarity of kmno4 solution is:
a)1
b)0.5
c)0.4
d)0.2
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I can't get the normality/milliequivalent of kmno4
I got it... wasn't getting the available weight of h2o2
To solve this problem, we need to use the concept of stoichiometry and molarity.
Let's break down the information provided:
1. We have a 3.4g sample of an H2O2 solution.
2. The concentration of H2O2 in the solution is x% by mass.
3. The reaction between H2O2 and KMnO4 occurs under acidic conditions.
4. We need to determine the molarity of the KMnO4 solution.
To approach this problem, we can follow these steps:
Step 1: Calculate the amount of H2O2 in grams from the given percentage.
To do this, we need to convert the percentage to a decimal and then multiply it by the total mass of the solution.
Given that the mass of the solution is 3.4g and the percentage is x%, the mass of H2O2 can be calculated as:
Mass of H2O2 = (x/100) * 3.4g
Step 2: Use stoichiometry to find the moles of H2O2.
Since the balanced equation between H2O2 and KMnO4 is not provided, we need to assume a balanced equation, which is typically:
5 H2O2 + 2 KMnO4 + 3 H2SO4 → 5 O2 + 2 MnSO4 + 8 H2O + K2SO4
According to this equation, 5 moles of H2O2 react with 2 moles of KMnO4. Therefore, we can calculate the moles of H2O2 as:
Moles of H2O2 = (Mass of H2O2) / (Molar mass of H2O2)
Step 3: Determine the moles of KMnO4 required.
Using the stoichiometry from the balanced equation, we know that 5 moles of H2O2 react with 2 moles of KMnO4. Therefore, moles of KMnO4 needed can be calculated as:
Moles of KMnO4 = (Moles of H2O2) * (2/5)
Step 4: Calculate the volume of KMnO4 solution in liters using molarity.
Molarity (M) is defined as moles of solute per liter of solution. Therefore, the volume of KMnO4 solution, in liters, can be calculated as:
Volume of KMnO4 (in L) = (Moles of KMnO4) / (Molarity of KMnO4 solution)
Now, let's apply these steps to solve the problem:
Step 1: Mass of H2O2 = (x/100) * 3.4g
Step 2: Moles of H2O2 = (Mass of H2O2) / (Molar mass of H2O2)
Step 3: Moles of KMnO4 = (Moles of H2O2) * (2/5)
Step 4: Volume of KMnO4 (in L) = (Moles of KMnO4) / (Molarity of KMnO4 solution)
Using these steps, we can calculate the volume of KMnO4 in liters. The answer choice that matches this calculated volume is the correct molarity of KMnO4 solution.