Answered: titration

Science

Chemistry

titration

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section16.3: Titrations And Buffers

Problem 2RQ

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Similar questions

Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
Which of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.
a.Calculate the pH of a buffer that is 0.1M in lactic acid, C2H4(OH)COOH, and 0.1M in sodium lactate, C2H4(OH)COONa. b.What is the pH of a buffer that is 1M in lactic acid and 1M in sodium lactate? c.What is the difference between the buffers described in parts a and b?
Explain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.
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.
Explain why the hydrolysis of salts makes it necessary to have available in a laboratory more than one acid-base indicator for use in titrations.
You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
Explain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it cannot be a buffer.
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
When titrating 50mL of 0.2MHCl, what quantity of 0.5M NaOH is needed to bring the solution to the equivalence point? a.80mL b.40mL c.20mL d.10mL
1. The titration curve shown at right represents which type of reaction? (a) A strong acid added to a strong base. (b) A strong base added to a strong acid. (c) A strong acid added to a weak base (d) A strong base added to a weak acid. volume of titrant added (from buret) pH of flask