A 27.00 mL volume of a monoprotic acid is titrated with 0.1723 M sodium hydroxide (NaOH). If 38.45 mL NaOH are required to reach the equivalence point, what was the original molar concentration (mol/L) of the acid? The reaction of the acid and the NaOH is:HA + NaOH = A- + H+ + H2O I got 0.2454 mol/L. Is that wrong?
A 27.00 mL volume of a monoprotic acid is titrated with 0.1723 M sodium hydroxide (NaOH). If 38.45 mL NaOH are required to reach the equivalence point, what was the original molar concentration (mol/L) of the acid? The reaction of the acid and the NaOH is:HA + NaOH = A- + H+ + H2O I got 0.2454 mol/L. Is that wrong?
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 27.00 mL volume of a monoprotic acid is titrated with 0.1723 M sodium hydroxide (NaOH).
If 38.45 mL NaOH are required to reach the equivalence point, what was the original molar concentration (mol/L) of the acid?
The reaction of the acid and the NaOH is:
HA + NaOH = A- + H+ + H2O
I got 0.2454 mol/L. Is that wrong?
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