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. Part A Part B Part C Part D • Part E Part F the pH after adding 6.0 mL of acid beyond the equivalence point Express your answer using two decimal places.

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. Part A Part B Part C Part D • Part E Part F the pH after adding 6.0 mL of acid beyond the equivalence point Express your answer using two decimal places.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.58QE

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Consider the titration of a 26.0 – mL sample of
0.180 M CH, NH, with 0.150 M HBr.
Determine each of the following.
Part A
Part B
Part C
Part D
Part E
Part F
the pH after adding 6.0 mL of acid beyond the equivalence point
Express your answer using two decimal places.
pH = 1.92
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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.
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. 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.
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A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.