Solved Example Acid-Base Titration
Example 1: A 25 mL solution of 0.5 M NaOH is titrated until neutralized into a 50 mL sample of HCl. Determine the concentration of the HCl solution.
Solution:
The concentration of the HCl solution is calculated to be 0.25 M through titration.
Example 2: A 30 mL solution of 0.2 M HCl is titrated with 0.15 M NaOH. Calculate the volume of NaOH required to reach the equivalence point.
Solution:
Using the formula MacidVacid = MbaseVbase
0.2 × 30 = 0.15 × Vbase
(0.2 × 30) ÷ 0.15 = Vbase
Vbase = 40ml
Hence, the volume of NaOH required is 40 ml.
Example 3: Titrate a 40 mL acetic acid (CH3COOH) solution with a 0.1 M NaOH solution. Determine the pH at the half-equivalence point.
Solution:
At the half-equivalence point, half of the acetic acid has reacted with NaOH, forming equal amounts of acetic acid and acetate ions, leading to a buffer solution with a specific pH value.
Acid Base Titration
Acid Base titration is a fundamental method in the quantitative chemical analysis used to determine the concentration of acids or bases in a solution. This process involves the controlled addition of a known concentration of an acid or base (titrant) to a solution of the substance being analyzed until the reaction reaches a neutral point. The moles of acid and base are equal at this equivalence point, resulting in a neutral solution. A pH indicator is often used to monitor the progress of the reaction, and a titration curve can be constructed to visualize the pH changes throughout the titration process.
In this article, we look into what is acid-base titration, titration curve, choice indicator, etc.
Table of Content
- What is Acid Base Titration?
- Titration Curve, Endpoint and Equivalence Point
- Choice of Indicators
- What Are Acid-Base Indicators?
- Use of Acid Base Titration
- Types of Acid Base Titrations