Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already addedenough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer shouldbe equal to 4.5.Values of K, for Some Common Weak BasesConjugateAcidNameFormulaKbAmmoniaNH3NH4+1.8 x 10-5Methylamine CH;NH,CH3NH3+4.38 x 10-45.6 x 10-4EthylamineC₂H5NH₂C₂H5NH3+AnilineCcHsNH₂CH5NH3+3.8 x 10-10PyridineC,H,NCH,NH*1.7 x 10-⁹1. Compute the poH of the buffer solution.

We know, [H+] ×[0H-] = 10-14 Or, log ( [H+] ×[OH-] ) =log…

Answered: - Compute the poH of the buffer…

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- Compute the poH of the buffer solution.

Chemistry

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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

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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

Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added
enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should
be equal to 4.5.
Values of K, for Some Common Weak Bases
Conjugate
Acid
Name
Formula
Kb
Ammonia
NH3
NH4+
1.8 x 10-5
Methylamine CH;NH,
CH3NH3+
4.38 x 10-4
5.6 x 10-4
Ethylamine
C₂H5NH₂
C₂H5NH3+
Aniline
CcHsNH₂
CH5NH3+
3.8 x 10-10
Pyridine
C,H,N
CH,NH*
1.7 x 10-⁹
1. Compute the poH of the buffer solution.

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