According to Arrhenius theory, acids are substances that dissociate in water to give hydrogen ions H+(aq) and bases are substances that produce hydroxyl ions OH–(aq). The ionization of an acid HX(aq) can be represented by the following equations: HX(aq) → H+(aq) + X–(aq) or HX(aq) + H2O(l) → H3O+(aq) + X–(aq) Similarly, a base molecule like MOH ionizes in aqueous solution according to the equation: MOH(aq) → M+(aq) + OH–(aq) Bronsted acids are proton donors whereas Bronsted bases are proton acceptors. Acids on donating proton form conjugate bases whereas bases form conjugate acids after accepting proton. Buffer solution is a solution whose pH does not change. By adding small amount of H+ or OH-. The decrease in concentration of the ion by adding other ion as common ion is called common ion effect. Ksp (solubility product) is product of molar concentrations of ions raised to power no. of ions per formula of ions per formula of the compound in sparingly soluble salt. Precipitation occurs only if ionic product exceeds solubility product. Solubility of salt decreases in presence of common ion. Kw the ionic product of water is 1×10⁻¹⁴ at 298 K. Kw increases with increase in temperature. pH is –log[H3O+] where [H3O+]=cα in monoprotic acid, c is molar conc., α is degree of ionisation.

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CASE_STUDIESArrhenius Concept of Acids and BasesBronsted-Lowry Concept of Acids and BasesIonic Product of Water KwCommon Ion Effect in Ionic EquilibriumBuffer Solutions and Their ActionSolubility Product Constant Ksp4 sub-questions

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