Acid-Base Titration Lab Report

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Determination of pKa and pKb Using Acid-Base Titrations Lab Report
This experiment aims at determining the concentration of acid-base equilibrium constants for acetic acid and aqueous ammonia using titration curves.
The main objective in the volumetric titration of an acid with a base is the determination of the equivalence point. The equivalence point is a point where the acid has been fully neutralized by the base. One can determine the completeness of the reaction by adding an indicator that changes when the reaction is approaching an equivalence point. Furthermore, the completeness of a reaction can be determined by a pH meter. A pH meter measures the actual pH of the solution during titration. pH titration
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A graduated cylinder was used to add 10ml of distilled water into a 100ml volumetric flask. 5.0ml concentrated acetic acid was pipetted into a 100ml volumetric which already had 10ml of distilled water. After adding acetic acid, the volumetric swirled to thoroughly mix the solution. The volumetric flask was then topped to the mark with distilled water and covered.
(2) Titration of Acetic Acid with Sodium Hydroxide
10ml of distilled water was added into a 250ml Erlenmeyer flask. 20ml of diluted acetic acid was then added into it, followed by setting up a titration system with 0.100M of NaOH in buret. A pH meter was used to monitor the pH of the solution as the base (NaOH) was added. Sodium hydroxide was added in an increment of 1ml until the solution pH reached 4.8. After the solution pH reached, the base was added in an increment of 0.2ml until the equivalence point was passed. After the equivalence point, the base was added in an internal of 1ml until there was an insignificant change in the solution pH. The volume of the base and pH of the solution were recorded and used to draw a titration

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