Is it likely easier to remove the first proton or second proton from the acid? Would this make the first constant larger or smaller? What conditions must exist to be able to ignore the second ionization?What simplifying assumptions do we usually make in working problems involving the ionization of a polyprotic acids? Why are they usually valid? Under what conditions do they fail? Answer by selecting all truestatements.The approximations are usually valid because the first ionization constant for the polyprotic acid is usually much larger than the second ionization constant.O The approximations are usually valid because the first ionization constant for the polyprotic acid is usually smaller than the second ionization constant.Nearly all of the Ht comes from the second ionization.Nearly all of the Ht comes from the first ionization.O If the first two ionization constants are not very different, the approximations fail.O If the first two ionization constants are not very different, the approximations are valid.The concentration of H* and the conjugate base of the polyprotic acid are approximately equal.O O O O O O

The question is based on the concept of polyprotic acids. there are certain approximations we make…

at simplifying assumptions do we usually make in working problems involving the ionization of a polyprotic acids? Why are they usually valid? Under what conditions do they fail? Answer by selecting all ements. The approximations are usually valid because the first ionization constant for the polyprotic acid is usually much larger than the second ionization constant. The approximations are usually valid because the first ionization constant for the polyprotic acid is usually smaller than the second ionization constant. Nearly all of the H* comes from the second ionization. Nearly all of the H* comes from the first ionization. If the first two ionization constants are not very different, the approximations fail. If the first two ionization constants are not very different, the approximations are valid. The concentration of H* and the conjugate base of the polyprotic acid are approximately equal.

at simplifying assumptions do we usually make in working problems involving the ionization of a polyprotic acids? Why are they usually valid? Under what conditions do they fail? Answer by selecting all ements. The approximations are usually valid because the first ionization constant for the polyprotic acid is usually much larger than the second ionization constant. The approximations are usually valid because the first ionization constant for the polyprotic acid is usually smaller than the second ionization constant. Nearly all of the H* comes from the second ionization. Nearly all of the H* comes from the first ionization. If the first two ionization constants are not very different, the approximations fail. If the first two ionization constants are not very different, the approximations are valid. The concentration of H* and the conjugate base of the polyprotic acid are approximately equal.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 5QRT

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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

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Is it likely easier to remove the first proton or second proton from the acid? Would this make the first constant larger or smaller? What conditions must exist to be able to ignore the second ionization?
What simplifying assumptions do we usually make in working problems involving the ionization of a polyprotic acids? Why are they usually valid? Under what conditions do they fail? Answer by selecting all true
statements.
The approximations are usually valid because the first ionization constant for the polyprotic acid is usually much larger than the second ionization constant.
O The approximations are usually valid because the first ionization constant for the polyprotic acid is usually smaller than the second ionization constant.
Nearly all of the Ht comes from the second ionization.
Nearly all of the Ht comes from the first ionization.
O If the first two ionization constants are not very different, the approximations fail.
O If the first two ionization constants are not very different, the approximations are valid.
The concentration of H* and the conjugate base of the polyprotic acid are approximately equal.
O O O O O O

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