The Sodium sulfite reacts with potassium permanganate and sulfuric acid. Sodium sulfite, potassium permanganate and sulfuric acid (KMnO4 H2SO4 Na2SO3) are very common and well-known chemical all around the world. It’s also available in almost all chemistry laboratories. They react to form the potassium sulfate, Manganese(II) sulfate, water as well as sodium sulfate. On the other hand, the reaction is an Oxidation-reduction reaction.
About KMnO4 Na2SO3 H2SO4
Potassium permanganate is an inorganic chemical compound and medication. It is a strong oxidizing agent. KMnO4 is a salt consisting of K+ and MnO4 -1 ions and has the chemical formula KMnO4. It dissolves in water to give intensely pink or purple solutions. In Solid-state it forms prismatic purplish-black glistening crystals.
Sodium sulfite (sodium sulfite) is a soluble sodium salt of sulfurous acid (sulfite) with the chemical formula Na2SO3. It is a product of sulfur dioxide scrubbing, a part of the flue-gas desulfurization process. It is also used as a preservative to prevent dried fruit from discoloring, and for preserving meats. It is also used in the same way as sodium thiosulfate to convert elemental halogens to their respective hydrohalic acids, in photography and for reducing chlorine levels in pools.
Sulfuric acid is a mineral acid with molecular formula H₂SO₄. It is a colorless, odorless, and syrupy liquid that is soluble in water. In this reaction, it acts as an acidic medium only.
Sodium sulfite reacts with potassium permanganate and sulfuric acid
The Sodium sulfite reacts with potassium permanganate and sulfuric acid to form the potassium sulfate, Manganese(II) sulfate, water as well as sodium sulfate. The skeleton reaction –
KMnO4 + H2SO4 + Na2SO3 = K2SO4 + MnSO4 + Na2SO4 + H2O
Now by using the ion-electron method we can balance the Oxidation-Reduction reaction.
The Ion-electron method is a very effective method to balance equations of the Redox reactions.
from the skeleton reaction, we can see that –
The Oxidizing agent: KMnO4 or MnO4-1
The Reducing agent: SO32-
Reduction Half Reaction:
MnO4 -1 +5e + 8H+ = Mn2- + 4H2O … …. …. …. (1)
Oxidation Half Reaction:
SO32- – 2e + O2- = SO42- … … … … (2)
equation (1)x2 + (2)x5,
2MnO4 -1 +10e + 16H+ = 2Mn2- + 8H2O
5SO22- – 10e + 5O2-= 5SO4-2
2MnO4 -1 + 16H+ + 5SO32- + 5O2-= 2Mn2- + 8H2O + 5SO4-2
⇒ 2MnO4 -1 + 6H+ +10H+ + 5O2-+ 5SO32- = 2Mn2- + 8H2O + 5SO4-2
⇒ adding necessary ions and radicals we get,
⇒ 2KMnO4 + 3H2SO4 + 5H2O + 5Na2SO2 = K2SO4 + 2MnSO4 + 8H2O + 5Na2SO4
⇒ 2KMnO4 + 3H2SO4 + 5Na2SO2 = K2SO4 + 2MnSO4 + 5Na2SO4 + 3H2O
Click to readily understand ion-electron balancing redox reaction-