Revision Notes on Hydrogen:

Hydrogen Element:

• Atomic number = Mass Number = 1

• Isotopes of hydrogen:

  • ¹H₁ : Protium , Most abundant in nature
  • ²H_1: Deuterium (D), Component of heavy water.
  •  ³H₁ : Tritium (T) , Radioactive in nature

Dihydrogen:

a. Laboratory preparation:
Reaction of metals with acids. Zn + H⁺→ Zn²⁺+H₂
b. Commercial Preparation:

1. Electrolysis of acidified water

2. Electrolysis of warm aqueous Ba(OH) 2 between nickel electrodes.

3. By-product in the manufacture of NaOH and Cl2 by electrolysis of brine solution.

4. Reaction of steam and hydrocarbons at high temperatures

c. Properties:

• Reaction with halogen: H₂ +X₂→ 2HX          [X= F, Cl, Br, I]

• Reaction with oxygen:  H₂(g) +O₂(g) + Δ → 2H₂O(l)      ΔH⁰ = -285.9 kJ mol^-1

• Reaction with nitrogen:  3H₂(g) +N₂(g) + Δ → 2NH₃(l)      ΔH⁰ = -92 kJ mol^-1

• Reaction with alkali metals: 3H₂(g) +2M(g) + Δ → 2MX(s)          

Uses of Hydrogen: 

• Used for synthesis of ammonia and vanaspati fat and many other products.

• Used as rocket fuel.

• Used in hydrogen fuel cells.                         

Hard Water:

a) Water containing carbonate, chloride and sulphate salts of calcium and magnesium.

Temporary hardens is due to the presence of carbonate salts and can be removed by boiling or by adding lime water.

Ca(HCO3)₂ + Ca(OH)₂ → 2CaCO₃↓+2H₂O

Ca(HCO₃)₂ + Δ → 2CaCO₃↓+2H₂O +CO₂↑

Permanent hardness is due to presence of sulphate and chloride salts and can be removed by treatment with washing soda.

MCl₂ + Na₂CO₃ → MCO₃ ↓ + 2NaCl ( M= Mg, Ca)

MSO₄ + Na₂CO₃ → MCO₃ ↓ + Na₂SO₄ ( M= Mg, Ca)

b)Hard water forms scum/precipitate with soap:

Heavy water:

• Molecular formula: D₂O

• 10.68% denser than ordinary water

• Freezing point 3.8 ⁰C

• Unfit for drinking and causes sterility.

Hydrogen peroxide :

a. Preparation :

Lab Method :

Na₂O₂ (s) + H₂SO₄(aq) --> H₂O₂(aq) + Na₂SO₄(s)

BaO₂.8H₂O + H₂SO₄(aq) --> H₂O₂ (aq) + BaSO₄(s)

Anhydrous barium oxide is not used because the precipitated BaSO₄ forms a protective layer on the unreacted barium peroxide and thus prevents its further participation in the reaction. However it can be overcome by using phosphoric acid.

By Electrolysis: 

By the auto-oxidation of 2-ethyl anthraquinol. The net reaction is a catalytic union of H₂ and O₂ to yield hydrogen peroxide.

b. Properties

i) Unstable liquid, decomposes to give water and dioxygen and the reaction is slow in the absence of catalyst. It is catalysed by certain metal ions, metal powders and  metal oxides.

2H₂O₂ (l) →  2H₂O (l) + O₂ (g)

ii) It  is a very powerful oxidising agent and poor reducing agent.  

As oxidising agent

In acidic medium: H₂O₂ + 2H⁺ + 2e^- →  2H₂O

In basic medium :H₂O₂ + OH^- + 2e^- → 3OH^--

As reducing agent

In acidic medium: H₂O₂ → 2H⁺ + O₂ + 2e^-

In basic medium : H₂O₂ + 2OH^- → 2H₂O + O₂ + 2e^-

2Fe²⁺ + H₂O₂ + 2H⁺ → 2Fe³⁺ + 2H₂O

2MnO₄^- + 5H₂O₂ + 6H⁺ → 2Mn²⁺ + 8H₂O + 5O₂

Mn²⁺ + H₂O₂ --> Mn⁺⁴ + 2OH^-

2Fe³⁺ + H₂O₂ + 2OH^- → 2Fe²⁺ + 2H₂O + O₂

The oxidising property of hydrogen peroxide is put to use in the restoration of old paintings, where the original white lead paint has been converted to black PbS by the H₂S in the atmosphere. Hydrogen peroxide oxidises the black PbS into white PbSO₄.

      PbS(s) + 4H₂O₂ (aq) --> PbSO₄(s) + 4H₂O

       black                                  white

c. Tests :

• It liberates iodine from potassium iodide in presence of ferrous sulphate

• Acidified solution of dichromate ion forms a deep blue colour with H₂O₂ due to the formation of CrO₅. ,
  Cr₂O₇^2- + 4H₂O₂ + 2H⁺ →  2CrO₅­ +5H₂O

• With a solution of titanium oxide in conc.H₂SO₄, it gives orange colour due to the formation of pertitanic acid.
  Ti⁴⁺ + H₂O₂ + 2H₂O → H₂TiO₄ + 4H⁺