We appreciate your visit to In another experiment the student titrated 50 0 mL of 0 100 M HC2H3O2 with 0 100 M NaOH aq Calculate the pH of the. This page offers clear insights and highlights the essential aspects of the topic. Our goal is to provide a helpful and engaging learning experience. Explore the content and find the answers you need!
Answer :
Final answer:
The pH of the solution at the equivalence point can be determined by considering the reaction between HC2H3O2 and NaOH. The solution will be basic at the equivalence point, so the pH will be greater than 7. The correct answer is C) pH of 8.00.
Explanation:
The pH of the solution at the equivalence point can be determined by considering the reaction that occurs between HC2H3O2 (acetic acid) and NaOH (sodium hydroxide). At the equivalence point, the moles of HC2H3O2 will be equal to the moles of NaOH added. Since acetic acid is a weak acid, its conjugate base, C2H3O2-, will be present in the solution. At the equivalence point, the solution will contain only the conjugate base of acetic acid, which makes it basic. Therefore, the pH of the solution at the equivalence point will be greater than 7.
From the given information, the titration of 50.0 mL of 0.100 M HC2H3O2 with 0.100 M NaOH is similar to the titration of acetic acid (a weak acid) with NaOH (a strong base). The titration curve for this reaction has an equivalence point of 8.72 pH. Since the pH at the equivalence point of the given titration is expected to be greater than 7, the answer choice C) pH of 8.00 is the most accurate.
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