Question 5 (1 point)4) ListenIt is necessary to carry out the titration of NaOH with KHP in the presence of carbondioxide.A) TrueO B) FalseQuestion 6 (1 point)ListenThe heat (or enthalpy) of neutralization (AH) is the heat evolved when a weak acid and a strong acıd react toform a salt plus water.OA) TrueB) False

It is necessary to carry out the titration of NAOH with KHP in the presence of carbon dioxide. A) True B) False Question 6 (1 point) ) Listen The heat (or enthalpy) of neutralization (AH) is the heat evolved when a weak acid and a strong acid react to form a salt plus water. OA) True B) False

It is necessary to carry out the titration of NAOH with KHP in the presence of carbon dioxide. A) True B) False Question 6 (1 point) ) Listen The heat (or enthalpy) of neutralization (AH) is the heat evolved when a weak acid and a strong acid react to form a salt plus water. OA) True B) False

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 5RQ: Draw the general titration curve for a strong acid titrated by a strong base. At the various points...

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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.

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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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1. Which of the following is/are TRUE about equivalence and end points? I. The end point of a titration is reached when the titrant and analyte are stoichiometrically equal. II. When you are titrating a strong or weak acid with a strong base, the end point will always be faint pink using a phenolphthalein indicator. III. When you are titrating a strong or weak acid with a strong base, the volume needed to reach the end point will always be lower than that of the equivalence point. a.I, II and III b.II only c.III only d.I and III 2. All but one are the criteria why KHP is generally used as the primary standard in determining the actual concentration of the sodium hydroxide titrant: a.It is highly pure. b.It is hygroscopic. c.It is chemically stable. d. It is inexpensive.
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