5. Show that the product of the dissociation constant (Ka) of a weak acid and thehydrolysis constant (Kb) of its conjugate base is the ion product of water (Kw).6.Some biological acids are phosphoric acid derivatives and some are carboxylic acidderivative.i. Using phosphoric acid H3PO4, write and expression forа. стb.a, in terms of K,ii.Consider the speciation curve for H2CO; below and use it to estimate the Ka(acid dissociation constant) for the reaction: H2CO3 + HCO; +H*09080.7060.5040.3020.1101214Guy Sawle, http://www.ozekoi.com/relationship%20between%20pH.pdf

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Show that the product of the dissociation constant (Ka) of a weak acid and the hydrolysis constant (Kb) of its conjugate base is the ion product of water (Kw).

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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

5. Show that the product of the dissociation constant (Ka) of a weak acid and the
hydrolysis constant (Kb) of its conjugate base is the ion product of water (Kw).
6.
Some biological acids are phosphoric acid derivatives and some are carboxylic acid
derivative.
i. Using phosphoric acid H3PO4, write and expression for
а. ст
b.a, in terms of K,
ii.
Consider the speciation curve for H2CO; below and use it to estimate the Ka
(acid dissociation constant) for the reaction: H2CO3 + HCO; +H*
09
08
0.7
06
0.5
04
0.3
02
0.1
10
12
14
Guy Sawle, http://www.ozekoi.com/relationship%20between%20pH.pdf

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