Redox Titration & Potentiometric Virtual Laboratory

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Redox Titration & Potentiometric Virtual Lab EMF vs V

Quantitative Electron Transfer & Potentiometry for JEE & NEET

Electrochemical Cell Active www.chemca.in

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1. Redox System Configuration

Select Titration Couple Permanganometry: KMnO₄ vs FeSO₄ (Acidic) Dichrometry: K₂Cr₂O₇ vs FeSO₄ (Diphenylamine Indicator) Iodometry: Na₂S₂O₃ vs I₂ (Starch Indicator)

Burette (Titrant) 0.02 M KMnO₄

Beaker (Analyte) 0.1 M FeSO₄ (50 mL)

💡 n-Factor Analysis: $\text{MnO}_4^-$ undergoes 5-electron reduction ($\text{Mn}^{+7} \to \text{Mn}^{+2}$), so $0.02\text{ M} \text{ KMnO}_4$ equals $0.1\text{ N}$.

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2. Titrant Flow Desk

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3. Microscopic Species Watcher

Potentiometer (EMF) 0.770 V

Volume Added 0.00 mL

0 mL246810

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FeSO₄ Analyte

Visual Observation Indicator

Solution: Colorless

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4. Live Lab Log & Molecular Feed

>> Lab Initialized. Potentiometric electrodes activated.

Add titrant from burette to monitor EMF changes.

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5. Potentiometric Plotter

Extrapolations

Intersection Pt: 5.00 mL

Potential E (V) dE/dV Inflection

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Redox Equivalents Calculator

Verify molar relationships via $M_1V_1 \times n_1 = M_2V_2 \times n_2$. Leave one parameter blank to solve.

M₁ (Titrant)

n₁ (Titrant n-factor)

M₂ (Analyte)

n₂ (Analyte n-factor)

V₁ (Titrant added at Endpoint, mL)

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Redox Master Quiz

Score: 0/5

📖 Quantitative Chemistry: n-Factors, Nernst Calculations & Visual Indicators (JEE/NEET Core)

Mathematical Nernst Dynamics

The potential of a redox titration couple ($E$) updates continuously. Before equivalence, potential is dictated by the analyte redox couple. For instance, the $\text{Fe}^{3+}/\text{Fe}^{2+}$ couple:

$$E = E^\circ_{\text{Fe}^{3+}/\text{Fe}^{2+}} - 0.059 \log \frac{[\text{Fe}^{2+}]}{[\text{Fe}^{3+}]}$$

At the exact equivalence point, the potential represents the weighted average:

$$E_{\text{eq}} = \frac{n_1 E^\circ_1 + n_2 E^\circ_2}{n_1 + n_2}$$

Permanganate vs Dichromate n-Factors

The $n$-factor is the total number of electrons transferred per mole of substance:

• $\text{KMnO}_4$ in Acidic Medium: $n = 5$ ($\text{Mn}^{7+} \to \text{Mn}^{2+}$)
• $\text{KMnO}_4$ in Strongly Basic: $n = 1$ ($\text{MnO}_4^- \to \text{MnO}_4^{2-}$)
• $\text{KMnO}_4$ in Weakly Alkaline/Neutral: $n = 3$ ($\text{MnO}_4^- \to \text{MnO}_2$)
• $\text{K}_2\text{Cr}_2\text{O}_7$ in Acidic Medium: $n = 6$ ($\text{Cr}_2\text{O}_7^{2-} \to 2\text{Cr}^{3+}$)

Indicator Mechanics

• $\text{KMnO}_4$ (Self-Indicator): The first unreacted drop at endpoint leaves a permanent, faint pink color due to localized unreduced $\text{MnO}_4^-$.
• Diphenylamine (Redox Indicator): It is colorless in reduced form, but a trace excess of dichromate oxidizes it to an intense deep violet-blue.
• Starch (Specific Indicator): Interacts with $\text{I}_3^-$ to form a deep blue-black coordination complex. Instant color dissipation marks the endpoint.

💡 Diagnostic Toast Message

© 2026 Chemca Interactive Labs. Built for deep Volumetric and Potentiometric redox concept acquisition.

Created for www.chemca.in

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