Part DConsider the titration of a 26.0 – mL sample of0.180 M CH,NH2 with 0.150 M HBr.Determine each of the following.the pH at one-half of the equivalence pointExpress your answer using two decimal places.?pH = 7.00SubmitPrevious Answers Request AnswerX Incorrect; Try Again; 5 attempts remaining• Part Ethe pH at the equivalence pointExpress your answer using two decimal places,pH - 7.00SubmitPrevious Answers Request AnswerX Incorrect; Try Again; 5 attempts remaining

pH is used to identify acidity and basicity of an aqueous solution. It is the negative logarithm of…

Answered: Consider the titration of a 26.0 -mL…

Chemistry for Today: General, Organic, and Biochemistry

9th Edition

ISBN:9781305960060

Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Publisher:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.128E

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Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?

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Consider the titration of a 26.0 -mL sample of 0.180 M CH,NH2 with 0.150 M HBr. Determine each of the following.