Question

can someone help me answer these 5 questions and figire this graph out please?

Acid-Base Titration of a Weak Acid with a Strong Base: Determination of K. Introduction: You will be titrating a solution of a weak acid with 0.100 M NaOH, while monitoring the reaction using a pH meter. Weak acids have characteristic acid-ionization constants, K. The purpose of this lab is to use the titration to determine the value of this constant for the weak acid called “benzoic acid” (HC-H502). The reaction equation is below: HC,H,O2 + NaOH NaC-H502 + H2O The pH curve for titration of acetic acid (a weak acid related to benzoic acid) is shown below. It differs from the pH curve for a strong acid in a few key ways. pH Curve for Titration of HC HO with NaOH 2 3 2 14.00 12.00 ocas 10.00 рн 3Fquivalence Pont 8.00 Haway Point foH = akaj 6.00 eeee 4.00 998 2.00 000 000 40 on 5000 2000 1000 Wu une ol Nai Because the titration involves the creation of a salt of a weak acid, the salt itself acts as a weak base. So, unlike the titration of a strong acid, the "neutralization point" in the titration occurs at a basic pH. (The term "equivalence point" is sometimes used since the salt solution will not have a neutral pH of 7.) The equivalence point (and equivalence pH) of the titration can be determined from the pH curve by finding the curve's point of inflection. This will always correspond to the equivalence point, just as it does for titration of a strong acid.

Answer 1