Question 2
Differentiate between
(i) Electrolytes and Non-electrolytes
(ii) Strong and Weak electrolytes
(iii) Anode and Cathode
(iv) Electrolytic dissociation and ionization with suitable examples.
(i) Differences between Electrolytes and Non-electrolytes are:
| Electrolytes | Non-electrolytes |
|---|---|
| Chemical compound which conduct electricity in the fused or in aqueous solution state and undergo chemical decomposition due to the flow of current through it. | Chemical compound which do not conduct electricity in the fused or aqueous solution state and do not undergo chemical decomposition due to the flow of current through it. |
| Electrolytes are ionic compounds | Non-electrolytes are covalent compounds |
| Particles in Electrolytes – ions only or Ions and molecules only | Particles in non-electrolytes – Molecules only |
| Examples : Acids — dil. HCl, HNO3 H2SO4. Alkalis — KOH, NaOH solutions. Ionic salts — PbBr2 [molten], CuSO4 [aq.] | Examples : Pure or distilled water, Alcohol, Kerosene, Carbon disulphide, liquid carbon tetrachloride, sucrose, glucose, sugar solution. |
(ii) Differences between Strong and Weak electrolytes are:
| Strong electrolytes | Weak electrolytes |
|---|---|
| They are electrolytes which allow a large amount of electricity to flow through them and hence are good conductors of electricity. | They are electrolytes which allow small amount of electricity to flow through them and hence are poor conductors of electricity. |
| They are almost completely dissociated in fused or aqueous solution state. | They are partially dissociated in fused or aqueous soln. state. |
| Particles in strong electrolytes are mainly ions only | Particles in weak electrolytes are ions and unionized molecules. |
| Examples : Generally all strong acids and bases and most salts of strong acids. Acids: dil. HCl, H2SO4, HNO3, HBr, HI. Bases : NaOH, KOH, LiOH soln. Salts: NaCl, NaNO3, Na2SO4, CuCl2 | Examples : Generally all weak acids and bases and most salts of weak acids. Acids: Carbonic, Acetic, Oxalic, Formic. Bases: NH4OH, Ca(OH)2, Mg(OH)2. Salts: Sodium carbonate, bicarbonate, oxalate and formate aq. soln. |
(iii) Differences between Anode and Cathode are:
| Anode | Cathode |
|---|---|
| It is the electrode connected to the positive terminal of the battery | It is the electrode connected to the negative terminal of the battery. |
| Anions migrate to anode | Cations migrate to cathode. |
| The anions donate excess electrons to the anode and they are oxidised to neutral atoms. Hence, Anode is the Oxidising Electrode. | The cations gain excess electrons from the cathode and they are reduced to neutral atoms. Hence, Cathode is the Reducing Electrode. |
(iv) Differences between Electrolytic dissociation and ionization are:
| Electrolytic Dissociation | Ionization |
|---|---|
| It is a process which takes place in electrovalent compounds | It is a process which takes place in covalent compounds. |
| It involves separation of ions which are already present in an ionic compounds. | It involves formation of charged ions from molecules which are not in the ionic state. |
| PbBr2 (ionic) ⇌ Pb2+ + 2Br1- | HCl [aq.] (covalent) ⇌ H1+ + Cl1-. Ionization may also involve atoms changing into ions [e.g. Mg ⟶ Mg2+ + 2e-] |
Chapter Overview: Electrolysis
Electrolysis is the process of decomposing an ionic compound (electrolyte) by passing an electric current through it in its molten or aqueous state. The apparatus consists of an electrolyte, two electrodes (anode and cathode), and a battery. Cations migrate to the cathode (reduction) and anions migrate to the anode (oxidation). The chapter covers electrolysis of molten lead bromide, acidified water, aqueous copper sulphate (with different electrodes), and concentrated HCl. The selective discharge theory explains which ions are preferentially discharged at electrodes when multiple ions are present. The electrochemical series helps predict the order of discharge. Applications include electroplating, electrorefining of metals, and extraction of reactive metals (like aluminium from alumina). Students must write electrode reactions (half-equations) showing electron gain at cathode and electron loss at anode, and understand the difference between electrolytes and non-electrolytes. This chapter requires understanding both the theory and practical applications of electrolysis.
Key Definitions & Electrode Reactions
| Term | Definition |
|---|---|
| Electrolysis | Chemical decomposition of an electrolyte by passing electric current through it |
| Electrolyte | Substance that conducts electricity in molten or aqueous state and is decomposed |
| Cathode | Negative electrode; cations are reduced here (gain electrons) |
| Anode | Positive electrode; anions are oxidised here (lose electrons) |
| Selective Discharge | When multiple ions are present, the ion lower in the electrochemical series is discharged first |
| Electroplating | Coating a metal object with a thin layer of another metal using electrolysis |
| Strong Electrolyte | Completely ionised in solution (e.g., NaCl, HCl, NaOH) |
| Weak Electrolyte | Partially ionised in solution (e.g., CH3COOH, NH4OH) |
Must-Know Concepts
- Electrolysis of acidified water: Cathode: 4H+ + 4e− → 2H2↑; Anode: 4OH− → 2H2O + O2↑ + 4e−
- H2 and O2 are produced in 2:1 volume ratio at cathode and anode respectively
- CuSO4 with Cu electrodes: Cu deposited at cathode, Cu dissolved from anode (copper refining)
- CuSO4 with Pt/C electrodes: Cu deposited at cathode, O2 at anode, solution turns acidic
- Molten PbBr2: Cathode: Pb2+ + 2e− → Pb; Anode: 2Br− → Br2 + 2e−
- Non-electrolytes: sugar solution, alcohol, kerosene (no free ions)
- For electroplating: object to be plated = cathode, plating metal = anode, salt of plating metal = electrolyte
Electrolyte vs Non-Electrolyte
| Property | Electrolyte | Non-Electrolyte |
|---|---|---|
| Bonding | Ionic or polar covalent | Non-polar covalent |
| Ions | Contains free ions | No free ions |
| Conductivity | Conducts when molten/dissolved | Does not conduct |
| Examples | NaCl, HCl, CuSO4 | Sugar, alcohol, urea |
Important Diagrams to Practice
- Electrolysis cell setup with labelled anode, cathode, electrolyte, and battery
- Electrolysis of acidified water showing gas collection in inverted test tubes
- Electroplating setup (e.g., silver plating on a spoon)
- Electrolytic refining of copper
Common Mistakes
- Confusing anode (+) and cathode (−) in electrolysis (opposite of electrochemical cells)
- Writing "oxidation at cathode" (cathode is always reduction in electrolysis)
- Forgetting that solid ionic compounds do not conduct electricity (ions are not free to move)
- Not balancing electrons in half-equations
- Confusing electrolysis of CuSO4 with Cu electrodes vs inert electrodes (products differ)
Scoring Tips
- Always write separate half-equations for cathode and anode reactions with electron transfer shown
- Specify whether electrodes are active (Cu, Ag) or inert (Pt, graphite) as this affects products
- For electroplating questions, clearly state: cathode = object, anode = plating metal, electrolyte = salt
- Remember: OILRIG (Oxidation Is Loss, Reduction Is Gain of electrons)
Frequently Asked Questions
Why is dilute H2SO4 added to water during electrolysis?
Pure water is a very poor conductor of electricity. Adding dilute H2SO4 increases the number of H+ and OH− ions, making the solution a better conductor. The acid itself is not consumed in the process.
Why does the colour of CuSO4 solution fade during electrolysis with inert electrodes?
Cu2+ ions (which give the blue colour) are deposited as copper metal at the cathode. Since the anode is inert, no copper dissolves to replace the Cu2+ ions, so the solution gradually becomes colourless and acidic (H2SO4 remains).
How is aluminium extracted by electrolysis?
Aluminium is extracted from purified alumina (Al2O3) dissolved in molten cryolite (Na3AlF6) by electrolysis. Cryolite lowers the melting point from 2050°C to about 950°C. At cathode: Al3+ + 3e− → Al. At anode: 2O2− → O2 + 4e−.