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Ch.8 - Monoprotic Acid-Base EquilibriaWorksheetSee all chapters

# Weak Acid-Base Equilibria

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Sections
Arrhenius Acids and Bases
Bronsted-Lowry Acids and Bases
Lewis Acids and Bases
Auto-Ionization
Ka and Kb of compounds
Weak Acid-Base Equilibria
Ionic Salts of Weak Acids and Bases
Buffers

WEAK ACIDS and WEAK BASES are weak electrolytes that do not completely ionize in solution, but instead form an equilibrium.

###### Weak Acid-Base Equilibria

Example #1: What is the original molarity of a solution of weak acid with a Ka of 4.7 x 10-3 and pH of 4.12 at 25 oC?

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Example #2: You are seeking to identify an unknown monoprotic acid by determining its Ka value. A 6.05 x 10-2 M solution of this unknown monoprotic acid has a pH of 2.122. Determine the Ka of this unknown acid?

a) 4.47 x 10-4
b) 9.42 x 10-4
c) 2.85 x 10-2
d) 1.08 x 10-3
e) 3.58 x 10-1

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Example #3: A weak acid has a pKa of 5.35. What is the hydronium ion concentration in a 0.10 M solution of this weak acid?

a) 5.4 x 10-4 M

b) 6.3 x 10-6 M

c) 3.5 x 10-5 M

d) 2.3 x 10-6 M

e) 4.5 x 10-6 M

f) 6.7 x 10-4 M

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Practice: The pH of an aqueous 0.10 M nitrite ion is 8.17. What is the base dissociation constant of the base?

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