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A solution is prepared by dissolving 1.9103 moles of H2SO4 and 3.4103 moles of HCl (two strong electrolytes) in 1kg of water at 298K and 1atm. Using the Debye-Hckel limit law, compute the activity of the cations in the solution. The equilibrium constant for the formation of ion pairs (i.e., the "association") in CuSO4 is Kao=230, in water at 25C. Calculate the molality of free Cu2+ ions in a solution prepared initially with a molality of 0.025mol/kg of solide CuSO4. (a) The equilibrium constant for the solubility of CaF2(s) (or "product of solubility") in water is K0=Kps=3.21011 at 25C and 1atm. Determine the solubility of CaF2(s) in pure water. (Neglect the formation of ion pairs, and use the Debye-Hckel limit law.) (b) Repeat the analysis in (a) for the solubitity of CaF2 in a 0.021 molal solution of KNO3 at the same temperature and pressure. (Note that Ca(NO3)2 is very soluble!)