A. start by assuming that when the reaction gets to equilibrium, the change in concentration of h+ will be negligible relative to the initial concentration. what do you get for [h+] and ph? report the concentration in scientific notation with the following format #*10^x (e. g. 0.0010 = 1.0*10^-3). [h+] = m ph = b. if you then use the quadratic formula, what do you get for your answers? report the concentration in scientific notation with the following format #*10^x (e. g. 0.0010 = 1.0*10^-3). [h+] = m ph = c. what is the % difference between the ph of (a) and (b)? calculate this by taking the larger of the two numbers and dividing it by the other, multiplying by 100, and then subtracting 100%. round this value to 2 sig figs. % difference = % d. [why are the two numbers different? ] e. if instead of a solution of benzoic acid, you had a solution of sodium benzoate, what do you get for [h+] and ph? report the concentration in scientific notation with the following format #*10^x (e. g. 0.0010 = 1.0*10^-3).