Electrolysis is one of the most important applications of electrochemistry taught in senior secondary chemistry, and silver nitrate serves as a classic example to understand electrode processes clearly. When aspirants prepare for numerical and conceptual questions, Silver nitrate electrolysis mcqs chemistry becomes a highly searched topic because it combines Faraday’s laws, electrode reactions, and practical observations into a single framework. A strong conceptual grasp of this system makes problem-solving much easier.

In aqueous silver nitrate electrolysis, silver nitrate dissociates completely into Ag⁺ and NO₃⁻ ions. The behavior of these ions during electrolysis explains why Silver nitrate electrolysis mcqs chemistry is frequently used to test understanding of selective discharge of ions. Silver ions have a high reduction potential, which makes them preferentially reduced at the cathode compared to hydrogen ions from water.

At the cathode, Ag⁺ ions gain electrons and get reduced to metallic silver. This deposition of silver is smooth, visible, and measurable, which is why silver nitrate is widely used in electroplating and laboratory demonstrations. Most Silver nitrate electrolysis mcqs chemistry questions rely on this predictable cathodic reaction to calculate mass deposited using Faraday’s laws.

The anode reaction depends on the nature of the electrode. When inert electrodes such as platinum or graphite are used, nitrate ions do not get oxidized. Instead, water molecules lose electrons to produce oxygen gas and hydrogen ions. This distinction is essential, as many Silver nitrate electrolysis mcqs chemistry problems test whether aspirants incorrectly assume nitrate oxidation at the anode.

Faraday’s first law of electrolysis states that the mass of a substance deposited is directly proportional to the quantity of electricity passed. This principle is central to numerical applications in Silver nitrate electrolysis mcqs chemistry, where current, time, and charge are linked to the amount of silver deposited. Since silver has a valency of +1, calculations become straightforward compared to multivalent metals.

Another reason Silver nitrate electrolysis mcqs chemistry is popular is its usefulness in comparing electrolysis outcomes with different electrolytes. When silver nitrate is electrolyzed, silver deposition occurs readily, unlike alkali metal nitrates where hydrogen evolution dominates. This contrast strengthens conceptual clarity about reduction potentials.

In silver nitrate electrolysis mcqs chemistry, electrolysis of silver nitrate also reinforces the understanding of oxidation and reduction. Oxidation always occurs at the anode and reduction at the cathode, regardless of the electrolyte used. Many Silver nitrate electrolysis mcqs chemistry questions are designed to catch mistakes related to electrode polarity and reaction direction.

In quantitative problems, aspirants often calculate the mass of silver deposited for a given current and time, or determine the current required for depositing a known mass. These applications make Silver nitrate electrolysis mcqs chemistry an ideal topic to test numerical accuracy along with theory. Since silver has a known atomic mass and simple electron exchange, it reduces computational errors.

Silver nitrate eletrolysis mcqs chemistry topic also helps bridge electrolysis with electrochemical equivalents and Faraday constants. Repeated exposure through Silver nitrate electrolysis mcqs chemistry strengthens familiarity with standard values like 96500 C per mole of electrons. This familiarity is crucial for speed and accuracy in competitive exams.

Another conceptual layer involves understanding why silver nitrate solutions are preferred in coulometric analysis. The clean deposition of silver without side reactions makes it reliable, which is why Silver nitrate electrolysis mcqs chemistry often appears in applied chemistry contexts as well.

From a broader exam perspective, Silver nitrate electrolysis mcqs chemistry integrates multiple chapters—electrochemistry, redox reactions, and stoichiometry—making it a high-value topic. Mastering the underlying concepts through silver nitrate electrolysis mcqs chemistry ensures aspirants can handle both direct and application-based questions confidently.

Silver nitrate electrolysis mcqs chemistry :

1.  4.5 g of aluminum (at. mass 27 amu) is deposited at cathode from Al³⁺ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H⁺ ions in solution by the same quantity of electric charge will be
   a) 44.8 L
   b) 22.4 L
   c) 11.2 L
   d) 5.6 L
   Answer: d

2. The electrode potentials for Cu²⁺(aq) + e⁻ → Cu⁺(aq) and Cu⁺(aq) + e⁻ → Cu(s) are +0.15 V and +0.50 V, respectively. The value of E°(Cu²⁺/Cu) will be
   a) 0.500 V
   b) 0.325 V
   c) 0.650 V
   d) 0.150 V
   Answer: b

3. The emf of a particular voltaic cell with the cell reaction Hg₂²⁺ + H₂ ⇌ 2Hg + 2H⁺ is 0.65 V. The maximum electrical work of this cell when 0.5 g of H₂ is consumed
   a) -3.12 × 10⁴ J
   b) -1.25 × 10⁵ J
   c) 2.50 × 10⁵ J
   d) None
   Answer: a

4. The standard reduction potential for Cu²⁺/Cu is +0.34. Calculate the reduction potential at pH = 14 for the above couple. (Ksp of Cu(OH)₂ = 1 × 10⁻¹⁹)
   a) 0.22 V
   b) -0.22 V
   c) -0.44 V
   d) 0.44 V
   Answer: b

5. For hydrogen-oxygen fuel cell, the cell reaction is 2H₂(g) + O₂(g) → 2H₂O(l). If ΔG°f(H₂O) = -237.2 kJ mol⁻¹, then emf of this cell is
   a) 2.46 V
   b) -2.46 V
   c) 1.23 V
   d) -1.23 V
   Answer: c

6. MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O; E° = 1.51 V, MnO₂ + 4H⁺ + 2e⁻ → Mn²⁺ + 2H₂O; E° = 1.23 V. E°(MnO₄⁻/MnO₂) is
   a) 1.70 V
   b) 0.91 V
   c) 1.37 V
   d) 0.548 V
   Answer: a

7. For the cell reaction 2Ce⁴⁺ + Co → 2Ce³⁺ + Co²⁺, E°cell is 1.89 V. If E(Co²⁺/Co) is -0.28 V, what is the value of E°(Ce⁴⁺/Ce³⁺)?
   a) 0.28 V
   b) 1.61 V
   c) 2.17 V
   d) 5.29 V
   Answer: b

8. Which of the following reaction is possible at anode?
   a) Fe²⁺ + 2e⁻ → Fe⁻
   b) 2H⁺ + (1/2)O₂ + 2e⁻ → H₂O
   c) 2Cr³⁺ + 7H₂O → Cr₂O₇²⁻ + 14H⁺ + 6e⁻
   d) None of the above
   Answer: c

9. Identify the incorrect statement for the given cell (image-based):
   a) If Eext > 1.1 V, Zn dissolves at Zn electrode and Cu deposits at Cu electrode
   b) If Eext = 1.1 V, no flow of electrons or current occurs
   c) If Eext > 1.1 V, electrons flow from Cu to Zn
   d) If Eext < 1.1 V, Zn dissolves at anode and Cu deposits at cathode
   Answer: a

10. Will MnO₄⁻ liberate O₂ from water in presence of an acid (given half-cells)?
    a) No, because E°cell = -2.733 V
    b) Yes, because E°cell = +0.287 V
    c) No, because E°cell = -0.287 V
    d) Yes, because E°cell = +2.733 V
    Answer: b

11. The amount of charge in F (Faraday) required to obtain one mole of iron from Fe₃O₄ is (Nearest integer)
    a) 2 F
    b) 3 F
    c) 4 F
    d) 5 F
    Answer: b

12. In two separate experiments, the same quantity of electricity was passed through silver and gold solutions (t constant). Ag and Au deposited are 2.15 g and 1.31 g. Valency of gold is
    a) 1
    b) 2
    c) 3
    d) 4
    Answer: c

13. If 5 ampere current is passed for 193 seconds through a solution containing copper salt, 0.32 g of copper is deposited. Oxidation state of Cu in the salt is
    a) 2
    b) 1
    c) 3
    d) 4
    Answer: a

14. A certain quantity of electricity is passed through aqueous Al₂(SO₄)₃ and CuSO₄ solutions in series. 0.09 g Al is deposited. Amount of Cu deposited is
    a) 0.318
    b) 3.18
    c) 0.636
    d) 31.8
    Answer: a

15. When 9.65 C electricity is passed through AgNO₃ solution, amount of Ag deposited is
    a) 10.8 mg
    b) 5.4 mg
    c) 16.2 mg
    d) 21.2 mg
    Answer: a

16. Approximate quantity of electricity required to deposit all silver from 250 mL of 1 M AgNO₃ is
    a) 96500 C
    b) 24125 C
    c) 48250 C
    d) 120625 C
    Answer: b

17. Time required to deposit all silver from 125 mL of 1 M AgNO₃ by passing current 241.25 A is
    a) 10
    b) 50
    c) 100
    d) 1000
    Answer: b

18. Assertion (A): A current of 96.5 A is passed into aqueous AgNO₃ solution for 100 s. The weight of silver deposited is 10.89 g (at. wt. of Ag = 108).
    Reason (R): The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.
    a) Both true and R explains A
    b) Both true but R not explanation
    c) A true but R false
    d) A false but R true
    Answer: c

19. Same quantity of electricity through AgNO₃ and H₂SO₄ in series. 5.04×10⁻² g H₂ liberated. Mass of Ag deposited is
    a) 0.54
    b) 5.4
    c) 10.8
    d) 5.04
    Answer: b

20. Acidified water electrolysis for 1930 s gives 1120 mL H₂ at STP. Current passed is
    a) 0.05
    b) 0.3
    c) 0.5
    d) 5
    Answer: d

21. For hypothetical reaction A → C (fast equilibrium A ⇌ B, slow step A + B → C). Rate law is
    a) ∝ [A][B]
    b) ∝ [A]²
    c) ∝ [A]²[B]²
    d) ∝ [A]²[B]
    Answer: a

22. Current 0.965 A for 2000 s through solution containing [Cu(CH₃CN)₄]⁺ deposits Cu. Amount deposited is
    a) 0.005 mol
    b) 0.01 mol
    c) 0.02 mol
    d) 0.04 mol
    Answer: c

23. Resistance of 0.1 M KCl in a conductance cell is 300 Ω, conductivity = 0.013 S cm⁻¹. Cell constant is
    a) 3.9 cm⁻¹
    b) 39 m⁻¹
    c) 0.39 cm⁻¹
    d) 3.9 m⁻¹
    Answer: a

24. Salts of A, B, C electrolyzed with same electricity. If 2.1 g of A deposited, B and C are 2.7 g and 9.6 g. Atomic masses 7, 27, 64. Valencies (A, B, C) are
    a) (3, 1, 2)
    b) (1, 3, 2)
    c) (3, 1, 3)
    d) (2, 3, 2)
    Answer: b

25. Constant current 30 A through aqueous NaCl for 1.00 h. Volume of Cl₂ at STP produced is
    a) 0.30 L
    b) 25.08 L
    c) 12.54 L
    d) 5.00 L
    Answer: c

26. Faradays needed to reduce 4 equivalents of Cu²⁺ to Cu is
    a) 1
    b) 2
    c) 4
    d) 8
    Answer: c

27. Electricity required to produce one mole of copper from CuSO₄ solution is
    a) 1 Faraday
    b) 2 Faraday
    c) 2.33 Faraday
    d) 1.33 Faraday
    Answer: b

28. Time (hours) required for 5.0 A to electroplate 60 g Ca from molten CaCl₂ is
    a) 27 hours
    b) 8.3 hours
    c) 11 hours
    d) 16 hours
    Answer: d

29. If 0.16 g Cu is deposited from CuSO₄, same charge through acidulated water gives H₂ volume at STP (Cu at. wt = 64)
    a) 4 cm³
    b) 56 cm³
    c) 60 cm³
    d) 8 cm³
    Answer: b

30. Which conversion involves gain of 5 electrons per ion?
    a) MnO₄⁻ → Mn²⁺
    b) CrO₄²⁻ → Cr³⁺
    c) MnO₄²⁻ → MnO₂
    d) Cr₂O₇²⁻ → 2Cr³⁺
    Answer: a

Conclusion on Silver Nitrate Electrolysis MCQs Chemistry

In conclusion, a thorough conceptual understanding of silver nitrate electrolysis mcqs chemistry simplifies exam preparation significantly. When aspirants clearly understand ion behavior, electrode reactions, and Faraday’s laws, Silver nitrate electrolysis mcqs chemistry becomes a scoring area rather than a confusing one. Repeated conceptual revision using Silver nitrate electrolysis mcqs chemistry , rather than rote memorization, is the key to mastering this topic effectively.