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A student was titrating a solution of hydrazine (H2NNHz) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 2 3 4 NEXT A 40.0 mL of 0.200 M H2NNH2 was titrated with 10 mL of 0.100 M HNO3 (a strong acid). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. H2NNH2(aq) + H(aq) H2NNH3(aq) Before (mol) Change (mol) After (mol) RESET 0 0.200 0.100 1.00 x 10 -1.00 x 10" 2.00 x 10" -2.00 x 10" 6.00 x 10" -6.00 x 10 7.00 x 10 -7.00 x 10" 8.00 x 10 8.00 x 10