Answer :
Final answer:
The pH of a 0.50 M Na2HA solution of a triprotic acid H3A, with respective pKa's of 5.00, 7.50, and 10.00, will be closest to the middle pKa, therefore the pH is 7.50.
Explanation:
The subject matter of the question revolves around the pH calculation for a triprotic acid, in this case, H3A. With given pKa's of 5.00, 7.50, and 10.00, each pKa corresponds to the dissociation of one proton. The pKa that will be closest to the pH of the solution will be the one with the concentration of the acid that is approximately 0.50 M. In this case, the middle pKa of 7.50 will be the closest, so the pH of the 0.50 M Na2HA solution of the triprotic acid H3A is 7.50.
Learn more about pH calculation here:
https://brainly.com/question/36153729
#SPJ11
