The solvation behaviour of chloramine-T in water and different compositions of water + co-solvent (dioxan, propan-2-ol and propan-1-ol) at 278, 288, 298 and 318K have been studied on the basis of conductivity principle. Experimentally obtained conductivity data are analysed by Kraus-Bray and Shedlovsky conductivity models to obtain limiting molar conductance, dissociation and association constants. Limiting molar conductance decreases with the increasing amount of co-solvent in water at all temperatures. Preferential solvation of cation by the co-solvent is identified. Thermodynamics of association in case of water + dioxan and dissociation in case of water + propan-2-ol and water + propan-1-ol are computed. Exothermic behaviour of solvation is observed. Ion pair formation constant (K-P) and triple ion formation constant (K-T) are determined from Fuoss-Accascina equation. K-P is found to be higher than K-T in all the cases, indicating the higher magnitude of association involved in the system. Solvation number is also calculated by a new model and is found to be fractional.