Assume that 30.0 mL of a 0.10 M solution of a weak base Bthat accepts one proton is titrated with a 0.10 M solutionof the monoprotic strong acid HA. (a) How many moles ofHA have been added at the equivalence point? (b) Whatis the predominant form of B at the equivalence point?(a) Is the pH 7, less than 7, or more than 7 at the equivalencepoint? (d) Which indicator, phenolphthalein or methylred, is likely to be the better choice for this titration?
Assume that 30.0 mL of a 0.10 M solution of a weak base Bthat accepts one proton is titrated with a 0.10 M solutionof the monoprotic strong acid HA. (a) How many moles ofHA have been added at the equivalence point? (b) Whatis the predominant form of B at the equivalence point?(a) Is the pH 7, less than 7, or more than 7 at the equivalencepoint? (d) Which indicator, phenolphthalein or methylred, is likely to be the better choice for this titration?
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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Assume that 30.0 mL of a 0.10 M solution of a weak base B
that accepts one proton is titrated with a 0.10 M solution
of the monoprotic strong acid HA. (a) How many moles of
HA have been added at the equivalence point? (b) What
is the predominant form of B at the equivalence point?
(a) Is the pH 7, less than 7, or more than 7 at the equivalence
point? (d) Which indicator, phenolphthalein or methyl
red, is likely to be the better choice for this titration?
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