10.Calculate the pH of the solution prepared by dissolving 0.48 mol of NH3(Kb=1.77x10-5) and 0.750 mol of ammonium chloride in enough water to make 1.00L of buffer solution Group of answer choices A, 5.09 B, 9.05 C, 9.44 D, no correct answer E, 10.1
10.Calculate the pH of the solution prepared by dissolving 0.48 mol of NH3(Kb=1.77x10-5) and 0.750 mol of ammonium chloride in enough water to make 1.00L of buffer solution Group of answer choices A, 5.09 B, 9.05 C, 9.44 D, no correct answer E, 10.1
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 34QRT
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10.Calculate the pH of the solution prepared by dissolving 0.48 mol of NH3(Kb=1.77x10-5) and 0.750 mol of ammonium chloride in enough water to make 1.00L of buffer solution
Group of answer choices
A, 5.09
B, 9.05
C, 9.44
D, no correct answer
E, 10.1
11,The equivalence point of titrating of the weak base with the strong acid will be observed at
Group of answer choices
A, pH>7
B, pH<7
C, pH=pKb
D, pH>pKb
E, pH=7
12,The titration curve of titrating a diprotic acid with a strong base will have two distinct equivalence points
Group of answer choices
A, if Ka1<<Ka2
B, if Ka1=Ka2
C, always
D, in case of ta strong acid
E, if Ka1>>Ka2
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