Practice: The pH of an aqueous 0.10 M nitrite ion is 8.17. What is the base dissociation constant of the base?
WEAK ACIDS and WEAK BASES are weak electrolytes that do not completely ionize in solution, but instead form an equilibrium.
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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