Nernst Equation: JEE Questions & Solutions

MX is a sparingly soluble salt that follows the given solubility equilibrium at 298 K. MX(s) ⇌ M^{+}(aq) + X^{-}(aq); K_sp = 10⁻¹⁰ If the…

Consider the following electrochemical cell at 298 K: Pt | HSnO₂⁻ (aq) | Sn(OH)₆²⁻ (aq) | OH⁻ (aq) | Bi₂O₃ (s) | Bi (s) If the reaction…

Consider the following electrochemical cell: Pt | O₂(g,1 bar) | HCl(aq) || M²⁺(aq,1.0 M) | M(s) The pH above which oxygen gas would start…

In the given electrochemical cell, Ag(s) | AgCl(s) | FeCl₂(aq), FeCl₃(aq) | Pt(s) at 298 K, the cell potential (E_cell) will increase when:…

Consider the above electrochemical cell where a metal electrode (M) is undergoing redox reaction by forming M⁺ (M → M⁺ + e⁻). The cation M⁺…

Consider the following redox reaction taking place in acidic medium: BH₄⁻ (aq) + ClO₃⁻ (aq) → H₂BO₃⁻ (aq) + Cl⁻ (aq) If the Nernst equation…

A volume of x mL of 5 M NaHCO₃ solution was mixed with 10 mL of 2 M H₂CO₃ solution to make an electrolytic buffer. If the same buffer was…

Based on the data given below: E^°_(Cr₂O₇²⁻/Cr³⁺) = 1.33 V, E^°_(Cl₂/Cl⁻) = 1.36 V, E^°_(MnO₄⁻/Mn²⁺) = 1.51 V, E^°_(Cr³⁺/Cr) = -0.74 V. The…

For a Mg | Mg²⁺(aq) || Ag⁺(aq) | Ag, the correct Nernst Equation is:

The standard reduction potential values of some of the p-block ions are given below. Predict the one with the strongest oxidising capacity.

Consider the following electrochemical cell at standard condition. Au(s) | QH₂, Q ∥ NH₄X (0.01 M) ∥ Ag⁺ (1 M) | Ag(s), E_cell = +0.4 V The…

1 Faraday electricity was passed through Cu²⁺ (1.5 M, 1 L)/Cu and 0.1 Faraday was passed through Ag⁺ (0.2 M, 1 L) electrolytic cells. After…

Consider the following half cell reaction Cr₂O₇²⁻ (aq) + 6e⁻ + 14H⁺ (aq) → 2Cr³⁺ (aq) + 7H₂O(1) The reaction was conducted with the ratio…

The hydrogen electrode is dipped in a solution of pH = 3 at 25^° C. The potential of the electrode will be - x × 10⁻² V.

Consider the cell: Pt(s)|H₂(g)(1 atm)|H⁺(aq,1 M)||Fe³⁺(aq),Fe²⁺(aq)|Pt(s) Given: E^°_(Fe³⁺/Fe²⁺) = 0.771 V, E^°_(H⁺/H₂) = 0 V, T = 298 K.…

Pt(s)|H₂(g)(1 bar)|H⁺(aq)(1 M)||M³⁺(aq), M⁺(aq)|Pt(s) The E_cell for the given cell is 0.1115 V at 298 K when [M⁺(aq)]/[M³⁺(aq)] = 10^a.…

The standard electrode potential (M³⁺/M²⁺) for V, Cr, Mn, and Co are -0.26 V, -0.41 V, +1.57 V, and +1.97 V, respectively. The metal ions…

Consider the cell Pt(s) | H₂ (g, 1 atm) | H⁺ (aq, 1 M) || Fe³⁺ (aq), Fe²⁺ (aq) || Pt(s). When the potential of the cell is 0.712 V at 298…

The electrode potential of the following half cell at 298 K. X | X²⁺ (0.001 M) ∥ Y²⁺ (0.01 M) | Y is..... × 10⁻² V (Nearest integer).…

At what pH, given half cell MnO₄⁻ (0.1 M) | Mn²⁺ (0.001 M) will have electrode potential of 1.282 V? \ (Nearest Integer) Given…

At 298 K, the standard reduction potential for the Cu²⁺/Cu electrode is 0.34 V. Given: K_sp(Cu(OH)₂) = 1 × 10⁻²⁰; take 2.303RT/F = 0.059 V.…