The student titrated 50.0 mL of 0.100 M HC2H3O2 with 0.100 M NaOH (aq). Calculate the pH of the solution at the equivalence point. Hd14T13-12-1110-9-8-7-6-5-4-3-322-1-5.0 10.0 15.0 20.0 25.0 30.0 35.0Volume of NaOH(aq) Added (mL)

pH of solution at equivalence point is 8.87.

Answered: The student titrated 50.0 mL of 0.100 M…

The student titrated 50.0 mL of 0.100 M HC2H3O2 with 0.100 M NaOH (aq). Calculate the pH of the solution at the equivalence point.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section: Chapter Questions

Problem 41PS

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

The student titrated 50.0 mL of 0.100 M HC₂H₃O₂ with 0.100 M NaOH (aq). Calculate the pH of the solution at the equivalence point.

Hd
14T
13-
12-
11
10-
9-
8-
7-
6-
5-
4-
3-
32
2-
1-
5.0 10.0 15.0 20.0 25.0 30.0 35.0
Volume of NaOH(aq) Added (mL)

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