Ncert Solutions Chemistry Class 11th

9.26. Water free from salts and minerals is called Demineralized water. Ion exchange method is used for this process. The ions present in the water bind to the positively or negatively charged sites on a resin when water is passed through the column packed with resin.

9.25. H₂O₂ as an oxidising agent:
2Fe²⁺  (aq) + 2H⁺ (aq) +H₂O₂ (aq) → 2Fe³⁺  (aq) + 2 H₂O (l)

H₂O₂ as a reducing agent:
I₂ (s) + H₂O₂  (aq) + 2OH^–  (aq) → 2I^–  (aq) + 2 H₂O (l) + O₂ (g)

9.24. Water is amphoteric in nature because it acts as an acid as well as a base.

Amphoteric nature of water is represented by following chemical reactions.

(1) Water as a base:
H_2?O(l)+H_2?S(g)?H₃?O⁺(aq)+HS⁻(aq)

(2) Water as an acid:
H_2?O(l) +NH₃?(aq)?OH⁻+NH₄⁺?

(3) Self ionization of water in which water simultaneously acts as acid and base.
2H₂?O→H

9.23. Cation exchange resins have large organic molecule with SO₃H group which are insoluble in water. Ion exchange resin (RSO₃H) is changed to RNa on treatment with NaCl. The resin exchange Na⁺ ions with Ca²⁺ and Mg²⁺ ions present in hard water and make it soft.
                                    2RNa (s) + M²⁺ (aq) ——> R₂M (s) + 2Na⁺ (aq)
where, M = Mg, Ca.
The resins can be regenerated by adding aqueous NaCl solution.

9.22. Temporary hardness of water is due to the presence of bicarbonates of calcium and magnesium in water i.e., Ca (HCO₃)₂ and Mg (HCO₃) in water. Permanent hardness of water is due to the presence of soluble chlorides and sulphates of calcium and magnesium i.e., CaCl₂, CaSO₄, MgCl₂ and MgSO₄.

9.21. Ice has crystalline structure which is highly ordered due to hydrogen bonding. It has hexagonal form at atmospheric pressure and cubic form at low temperature. Each O atom has tetrahedral geometry and is surrounded by 4 oxygen atoms each at a distance of 276 pm.

9.20.  (i) PbS(s) +4H₂O₂(aq) → PbSO₄(s) + 4H₂O(l)

(ii) 2MnO₄^– (aq) +H₂O₂(aq) + 6H⁺(aq) → 2Mn (aq) + 8H₂O(l) + 5O₂(g)

(iii) CaO(s) + H₂O(g) → Ca(OH)₂(aq)

(iv) AlCl₃(aq) + 3H₂O(l) → Al(OH)₃(s) + 3HCl (aq)

(v) Ca₃N₂(s) + H₂O(l) → 3Ca(OH)₂(aq) + 2NH₃(aq)

(a) Hydrolysis reactions, (iii) (iv) and (v)

(b) Redox reactions (i) and (ii)

9.19. 2F₂ (ag) + 2H₂O (l)? O₂ (g) + 4H⁺ (aq) + 4F (aq)
In this reaction water acts as a reducing agent and itself gets oxidised to O₂ while F₂ acts as an oxidising agent and hence itself reduced to F^– ions.

9.18. Auto-protolysis means self-ionisation of water. It may be represented as

2H₂O(l) + H₂O(l) ? H₃O⁺(aq) + OH^-(aq)

Acid 1       Base 2     Acid 2        Base 1
Due to auto-protolysis nature of water, it can act as an acid as well as base, i.e. amphoteric in nature.

9.17. In water, O is sp³ hybridized. Due to stronger lone pair-lone pair repulsions than bond pair-bond pair repulsions, the HOH bond angle decreases from 109.5° to 104.5°. Thus, water molecule has a bent structure.

H₂O₂ has a non-planar structure. The O—H bonds are in different planes. Thus, the structure of H₂O₂ is like an open book.