A weak base was titrated with 0.275 M HBr. 44.00 mL of the HBr solution was required to reach the equivalence point. During the titration, the pH after adding 5.50 mL of HBr was 7.088. Calculate the Kb for the weak base. (Hint: when you do a partial neutralization of a weak acid or base, the solution formed is usually a buffer)
A weak base was titrated with 0.275 M HBr. 44.00 mL of the HBr solution was required to reach the equivalence point. During the titration, the pH after adding 5.50 mL of HBr was 7.088. Calculate the Kb for the weak base. (Hint: when you do a partial neutralization of a weak acid or base, the solution formed is usually a buffer)
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 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...
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A weak base was titrated with 0.275 M HBr. 44.00 mL of the HBr solution
was required to reach the equivalence point. During the titration, the pH
after adding 5.50 mL of HBr was 7.088. Calculate the Kb for the weak base.
(Hint: when you do a partial neutralization of a weak acid or base, the
solution formed is usually a buffer)
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