Phosphoric acid (H3PO4, molecular weight =98g/mol) is added to pure water and the following reactions occur: H3PO4H2PO4HPO4H++H2PO4;pKa=2.12H++HPO42;pKa=7.20H++PO43;pKa=12.32 If the initial phosphoric acid concentration is 5.0g/L, what are the molar concentrations of H3PO4,H2PO3,HPO42,PO43, and H+at equilibrium in a water at 25C ? Please treat all three of these dissociations as a weak acids, and check that your assumptions for developing an ICE table are valid