(Solved): Don't know how to calculate the 3 equivalence points of this titration of H3PO4 with NaOH to be able ...

You need to graph \& fully interpret the pH titration curve. making note of the inflections, equivalence points, buffer regions, where \( \mathrm{pH}=\mathrm{pK}_{\mathrm{a}} \). You will need to make use of 'basic calculus' in order to accurately measure the volumes at the end-points. and thus determine the exact molarity of the phosphoric acid. Sample Data Iprovided below]: Note - Since the \( \mathrm{NaOH} \) and the \( \mathrm{H}_{3} \mathrm{PO}_{4} \) solutions are about the same strength, \( 0.100 \mathrm{M} \), the ratio of the volumes reacted should be the same as the ratio of the moles reacted (note: \( 10.00 \mathrm{ml} \) acid was used). For \( \mathrm{pH} \) titration - You will graph this data in Excel. Graph: Plot in Excel pH (ordinate, ie, y-axis) vs. volume of NaOH (abscissa, ic., x-axis). Show the data points, and then overlay the points with a best-fit polynomial line. Indicate on the plots. a) the buffer region(s), b) the region(s) where \( \mathrm{pH}=\mathrm{pKa} \), c) the end point(s), d) the region where \( \mathrm{OH}^{-} \)is in excess, and e) the maior species present in solution in each region. (acid. coniugate base. etc)