Given the following reversible reactions and Kc values: (I) Self-ionization of water:         H2O + H2O    H3O+ + OH-,   Kc = Kw = 1.0 x 10-14. (II) Ionization of a weak base:     NH3 + H2O    NH4+ + OH-,   Kc (= Kb) = 1.8 x 10-5. a) Determine the Kc­ for the reaction:                                     NH3 + H3O+  NH4+  +  H2O b)  Would you assess the Kc value as LARGE or small? Does your assessment make sense for this reaction, i.e. think about the species involved?

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3. Answer all sections (i) - (iv). 1 mole of ethanol (C2H5OH) and 1 mole of ethanoic acid (CH;COOH) were reacted at 25 °C, in a non- aqueous solvent, until equilibrium was reached. It was subsequently determined that 0.33 moles of ethanol remained at equilibrium. (i) Write an equation for the reaction. (ii) Write an expression for the equilibrium constant, Kc, for the reaction and calculate its value. Subsequently a further 3 moles of C2H5OH was added to the solution. (ii) Determine the concentrations of all the species present when equilibrium is restored.