a solution of arsenic oxide containing 0.24g required 50cm^3 of acidified potassium manganate of solution of concentration 0.02M for complete oxidation. What is the oxidation state of arsenic in the product?
Are you sure this is potassium manganate or should you have written potassium permanganate.
Potassium manganate 7
To find the oxidation state of arsenic in the product, we need to understand the reaction taking place.
From the information given, we know that a solution of arsenic oxide (As2O3) required an acidified potassium manganate (KMnO4) solution for complete oxidation. The reaction can be represented as follows:
2KMnO4 + 3H2SO4 + As2O3 → K2SO4 + 2MnSO4 + 3H2O + As2O5
Here, KMnO4 acts as an oxidizing agent, and As2O3 is getting oxidized to As2O5. The changes in oxidation states are as follows:
Initially, in As2O3, the oxidation state of As is +3, and in KMnO4, the oxidation state of Mn is +7.
After the reaction, in As2O5, we need to determine the oxidation state of As.
To calculate the oxidation state of As in As2O5, we need to understand that the sum of oxidation states in a compound is equal to the overall charge of the species.
In As2O5, oxygen has an oxidation state of -2 (almost always). And since the compound is neutral overall, the sum of the oxidation states should be zero.
Let's assume the oxidation state of As in As2O5 is X.
We have 2 As atoms, each with an unknown oxidation state X. We also have 5 oxygen atoms, each with an oxidation state of -2.
Using these values, we can set up an equation:
2X + 5(-2) = 0
Simplifying the equation:
2X - 10 = 0
2X = 10
X = 5/2
Therefore, the oxidation state of arsenic (As) in As2O5 is +5/2.
Please note that oxidation states can sometimes be fractional, indicating that the electron distribution is not well-defined and lies between two whole numbers.