What is the pH of a solution of Atropine (a weak base) if the concentration of nondissociated form of the drug is 0.526 M. (The pk, of the drug is 4.35 and its solubility at that pH is 0983 M). Oa. 9.65 O b. 9.71 C 9.13 d. 9.59

What is the pH of a solution of Atropine (a weak base) if the concentration of nondissociated form of the drug is 0.526 M. (The pk, of the drug is 4.35 and its solubility at that pH is 0983 M). Oa. 9.65 O b. 9.71 C 9.13 d. 9.59

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 78AP

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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.

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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

What is the pH of a solution of Atropine (a weak base) if the concentration of nondissociated
form of the drug is 0.526 M. (The pk, of the drug is 4.35 and its solubility at that pH is 0983
M).
Oa. 9.65
Ob.9.71
OC 9.13
d. 959

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