Our chemist found a solution of 0.333M H3PO4 (phosphoric acid) and another of 1.05M NaOH (amazing what you can find in the belly of a ship) and so she did an enthalpy of neutralization reaction using 50.0mL of each solution. (Phosphoric acid is a triprotic acid; each mole of acid can yield 3 moles of H+ ions.) Using the CRC Handbook at hand, the density and specific heats of the final solution were found to be 1.11 g/mL and 3.81 J/ g oC, respectively. From the graph of her results, she determined the average temperatures of the acid and basic solutions prior to mixing, an initial temperature of 20.1 oC. In the same manner, she determined that the neutralized solution, her product, reached a maximum temperature of 26.0 oC at the time of mixing.

A: Calculate the heat (in Joules) absorbed by the solution using the equation: ΔHrxn = Specific heat (CP) × Mass × ΔTrxn

B:Using the calorimeter constant, calculate the magnitude (i.e. absolute value only) of the heat lost to the environment, ΔHenv in Joules, for the reaction of phosphoric acid and sodium hydroxide. ΔHenv = Calorimeter constant × ΔTrxn

C:Calculate the ΔHneut in Joules using the equation: ΔHneut = ΔHrxn + ΔHenv