What are Lewis acids and bases? Give two example for each.

Indentify the conjugate acid base pair for the following reaction in aqueous solution
i) HS^- (aq) + HF \(\rightleftharpoons \) F^-(aq) + H₂S(aq)
ii) HPO^2-₄ + SO₃^2- \(\rightleftharpoons \) PO₄^3- + HSO₃^-
iii) NH₄⁺ + CO₃^2-  \(\rightleftharpoons \) NH₃ + HCO₃^-

Account for the acidic nature of HClO₄ in terms of Bronsted – Lowry theory, identify its conjugate base.

When aqueous ammonia is added to CuSO₄ solution, the solution turns deep blue due to the formation of tetra ammine copper (II) complex,\({ [Cu({ H }_{ 2 }O)_4] }_{ (aq) }^{ 2+ }+ 4{ NH }_{ 3 }(aq)\rightleftharpoons { [Cu{ ({ NH }_{ 3 }) }_{ 4 }] }_{ (aq) }^{ 2+ }\) among H₂O and NH₃ Which is stronger Lewis base.

Define solubility product.

Define pH.

K_sp of AgCl is \(1.8\times10^{-10}\). Calculate molar solubility in 1 M AgNO₃

Calculate the concentration of OH^- in a fruit juice which contains \(2\times10^{-3}\) M, H₃O⁺ ion. Identify the nature of the solution.

Calculate the pH of 0.001M HCl solution

A solution of 0.10M of a weak electrolyte is found to be dissociated to the extent of 1.20% at 25^oC. Find the dissociation constant of the acid.

Calculate the pH of 0.1M CH₃COOH solution. Dissociation constant of acetic acid is \(1.8\times10^{-5}\).