(a) Identify the conjugate acid-base pairs in these equilibria: (i) (CH3)3N+H2O(CH3)3NH++OH {21/2} (ii) NH2+H2ONH3+OH {21/2} (b) Balance the following redox equations: (i) SO32+MnO4+H2OMnO2+SO42+OH {21/2} (ii) Ag(s)+H+(aq)+NO3(aq)Ag+(aq)+NO2(g)+H2O (l) {221} (c) The concentrations of NaCl and KI are at 0.120M and 0.090M, respectively, in the following electrochemical cell: Cu(s)Cul(s)(aq)Cl(aq)AgCl(s)Ag(s) Using Nerst equation, calculate the cell voltage and solubility products (Ksp) for AgCl and Cul respectively using the following half-reactions: Cu++eCu(s)E0=0.518VAg++eAg(s)EO=0.7993V