Faculty of Technological Studies Uva Wellassa University
Department of Biosystems Technology
BST 121-3
Experiment no-05
Commercial Importance of Strong Base Weak Acid and Weak Base Strong Acid Titrations
Hashan shanaka kumarasinghe
BBST22065
Date 2024/02/14
Practical no -05
Practical name
Commercial Importance of Strong Base Weak Acid and Weak Base Strong Acid Titrations
Objectives
Understanding and demonstrating the titration procedures involving strong base weak acid and weak
base strong acid reactions is the aim of this experiment. In particular, we want to use titration
techniques to find the amounts of sodium bicarbonate in solution and acetic acid in vinegar.
Introduction
Titration is a fundamental technique in analytical chemistry used to determine the concentration of a
substance in solution by reacting it with a known concentration of another substance until a reaction
endpoint is reached. In this experiment, we explore the commercial importance of two types of
titrations: strong base with weak acid and weak base with strong acid.
The first part of the experiment involves titrating vinegar (acetic acid) with sodium hydroxide (NaOH), a
strong base. Acetic acid is a weak acid commonly found in household vinegar, while sodium hydroxide is
a strong base. The reaction between these compounds is represented as follows:
CH3COOH+NaOH→CH3COONa+H2O
The second part of the experiment focuses on titrating sodium bicarbonate (NaHCO3) with hydrochloric
acid (HCl), a strong acid. Sodium bicarbonate is a weak base, and the reaction with hydrochloric acid
produces sodium chloride, water, and carbon dioxide:
NaHCO3+HCl→NaCl+H2O+CO2
Two different indicators, phenolphthalein and methyl orange, are used in the second titration to
determine the endpoint based on color changes.
, Understanding these titration procedures is essential in a number of sectors, including pharmaceuticals,
environmental monitoring, and food and beverage. Accurately calculating the amounts of acid and base
guarantees high-quality products, effective processes, and adherence to regulations.
We highlight the commercial value of strong base weak acid and weak base strong acid titrations in this
study by presenting the experimental methodology, observations, calculations, and interpretations of
the titration results.
Materials
Vinegar (5 mL)
Sodium hydroxide (NaOH) solution, 0.1M
Hydrochloric acid (HCl) solution, 0.1M
Sodium bicarbonate (NaHCO3) (0.1 g)
Phenolphthalein indicator
Methyl orange indicator
Burette
Titration flask
Pipettes
Distilled water
Methodology
The solutions were prepared by mixing 5 mL of vinegar with 20 mL of distilled water to create the
vinegar solution, and 0.1 g of sodium bicarbonate (NaHCO3) was dissolved in 25 mL of distilled water to
prepare the sodium bicarbonate solution. The titration process for vinegar involved filling the burette
with 0.1M NaOH solution and transferring the prepared vinegar solution to the titration flask, where a
few drops of phenolphthalein indicator were added. The vinegar solution was titrated with NaOH
solution until a color change from pink to colorless indicated the endpoint, with the volume of NaOH
solution used recorded for each of the three trials conducted. For the sodium bicarbonate titration, the
burette was refilled with 0.1M HCl solution, and the prepared sodium bicarbonate solution was
transferred to a clean titration flask. Phenolphthalein indicator was used for one trial, while methyl
orange indicator was used for another trial. The sodium bicarbonate solution was titrated with HCl
solution until the color changes according to the indicator used, marking the endpoint, and the volumes
of HCl solution used were recorded for both indicators, with two trials conducted for each indicator.
Department of Biosystems Technology
BST 121-3
Experiment no-05
Commercial Importance of Strong Base Weak Acid and Weak Base Strong Acid Titrations
Hashan shanaka kumarasinghe
BBST22065
Date 2024/02/14
Practical no -05
Practical name
Commercial Importance of Strong Base Weak Acid and Weak Base Strong Acid Titrations
Objectives
Understanding and demonstrating the titration procedures involving strong base weak acid and weak
base strong acid reactions is the aim of this experiment. In particular, we want to use titration
techniques to find the amounts of sodium bicarbonate in solution and acetic acid in vinegar.
Introduction
Titration is a fundamental technique in analytical chemistry used to determine the concentration of a
substance in solution by reacting it with a known concentration of another substance until a reaction
endpoint is reached. In this experiment, we explore the commercial importance of two types of
titrations: strong base with weak acid and weak base with strong acid.
The first part of the experiment involves titrating vinegar (acetic acid) with sodium hydroxide (NaOH), a
strong base. Acetic acid is a weak acid commonly found in household vinegar, while sodium hydroxide is
a strong base. The reaction between these compounds is represented as follows:
CH3COOH+NaOH→CH3COONa+H2O
The second part of the experiment focuses on titrating sodium bicarbonate (NaHCO3) with hydrochloric
acid (HCl), a strong acid. Sodium bicarbonate is a weak base, and the reaction with hydrochloric acid
produces sodium chloride, water, and carbon dioxide:
NaHCO3+HCl→NaCl+H2O+CO2
Two different indicators, phenolphthalein and methyl orange, are used in the second titration to
determine the endpoint based on color changes.
, Understanding these titration procedures is essential in a number of sectors, including pharmaceuticals,
environmental monitoring, and food and beverage. Accurately calculating the amounts of acid and base
guarantees high-quality products, effective processes, and adherence to regulations.
We highlight the commercial value of strong base weak acid and weak base strong acid titrations in this
study by presenting the experimental methodology, observations, calculations, and interpretations of
the titration results.
Materials
Vinegar (5 mL)
Sodium hydroxide (NaOH) solution, 0.1M
Hydrochloric acid (HCl) solution, 0.1M
Sodium bicarbonate (NaHCO3) (0.1 g)
Phenolphthalein indicator
Methyl orange indicator
Burette
Titration flask
Pipettes
Distilled water
Methodology
The solutions were prepared by mixing 5 mL of vinegar with 20 mL of distilled water to create the
vinegar solution, and 0.1 g of sodium bicarbonate (NaHCO3) was dissolved in 25 mL of distilled water to
prepare the sodium bicarbonate solution. The titration process for vinegar involved filling the burette
with 0.1M NaOH solution and transferring the prepared vinegar solution to the titration flask, where a
few drops of phenolphthalein indicator were added. The vinegar solution was titrated with NaOH
solution until a color change from pink to colorless indicated the endpoint, with the volume of NaOH
solution used recorded for each of the three trials conducted. For the sodium bicarbonate titration, the
burette was refilled with 0.1M HCl solution, and the prepared sodium bicarbonate solution was
transferred to a clean titration flask. Phenolphthalein indicator was used for one trial, while methyl
orange indicator was used for another trial. The sodium bicarbonate solution was titrated with HCl
solution until the color changes according to the indicator used, marking the endpoint, and the volumes
of HCl solution used were recorded for both indicators, with two trials conducted for each indicator.
