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Step-by-step reaction balancers, 3D molecular coordinate viewers, and active recall practice engines for NEB Class 11–12 and IOE candidates.

ION-ELECTRON METHOD · ACIDIC MEDIUM

Step-by-Step Redox Reaction Balancer

Follow explicit oxidation state assignments, half-reaction splits, electron equalization, and mass conservation.

Full Screen Mode
Target Board ReactionAcidic Solution (H⁺ / H₂O)
KMnO4+FeSO4+H2SO4⟶MnSO4+Fe2(SO4)3+K2SO4+H2O\text{KMnO}_4 + \text{FeSO}_4 + \text{H}_2\text{SO}_4 \longrightarrow \text{MnSO}_4 + \text{Fe}_2(\text{SO}_4)_3 + \text{K}_2\text{SO}_4 + \text{H}_2\text{O}
Step 1 of 7

Assign Oxidation States & Identify Half-Reactions

Determine which element undergoes an increase in oxidation state (oxidation) and which undergoes a decrease (reduction).

Mn+7O4−+Fe+22+⟶Mn+22++Fe+33+\overset{+7}{\text{Mn}}\text{O}_4^- + \overset{+2}{\text{Fe}}^{2+} \longrightarrow \overset{+2}{\text{Mn}}^{2+} + \overset{+3}{\text{Fe}}^{3+}
Mn: +7→+2 (Gain of 5 e−, Reduction)∣Fe: +2→+3 (Loss of 1 e−, Oxidation)\text{Mn: } +7 \rightarrow +2 \text{ (Gain of 5 } e^-, \text{ Reduction)} \quad | \quad \text{Fe: } +2 \rightarrow +3 \text{ (Loss of 1 } e^-, \text{ Oxidation)}

Why this step matters

Redox reactions cannot be balanced by mere guesswork because electrons must be strictly conserved alongside mass. Identifying oxidation numbers isolates the true redox drivers from non-reacting spectator ions.

Key Chemical Principle

LEO says GER: Loss of Electrons is Oxidation (Reducing Agent), Gain of Electrons is Reduction (Oxidizing Agent).

Check Your Understanding

Which chemical species is oxidized and acts as the reducing agent in this reaction?

METHODOLOGY REFERENCE

Systematic Rules for Balancing in Acidic Medium

01 · OTHER ATOMS

Adjust stoichiometric coefficients for elements other than Oxygen and Hydrogen.

02 · OXYGEN (H₂O)

Add 1 molecule of H₂O on the deficient side for every oxygen atom needed.

03 · HYDROGEN (H⁺)

Add H⁺ ions on the deficient side to balance hydrogen atoms introduced by water.

04 · CHARGE (e⁻)

Add electrons (e⁻) to the more positive side until both sides possess equal net charges.