Lab Report Acid Base Titration
EXPERIMENT 3: INTRODUCTION TO TITRATION – DETERMINATION OF THE MOLARITY AND CONCENTRATION OF SULPHURIC ACID BY TITRATION WITH A STANDARD SOLUTION OF SODIUM HYDROXIDE
INTRODUCTION
Reaction of acid and base is one of the most common reaction in chemistry. This reaction is also widely known as neutralization. In this experiment, we used titration technique which involves accurately measuring the volume of a solution required to react with another reagent. An indicator must be used to determine the end point of the titration. The indicator used can change colors at different pH values.
OBJECTIVE
To determine the concentration of sulphuric acid (H2SO4) using titration technique
CHEMICALS
NaOH solution, approximately 0.2 M, dilute sulphuric acid of unknown molarity, phenolphthalein
APPARATUS
Burette. Burette clamp, retort stand, 20 mL volumetric pipette, pipette filter, 250 mL conical flask
PROCEDURES
1) The burette was washed with distilled water and then rinsed with about 5-10 mL of NaOH solution, running the second rinsing through the burette tip. The burette was clamped to the retort stand
2) The burette was filled with the base, made sure the tip was completely filled and contain no air bubbles. The initial burette reading was recorded
3) Using a volumetric pipette, 20.00 mL H2SO4 was transferred to a clean 250 mL conical flask. 2 or 3 drops of phenolphthalein indicator was added. This flask was placed on a piece of white paper under the burette and the burette tip was lowered into the flask. The initial burette reading was recorded, to 2 decimal places
4) The acid was titrated by adding base until the end point was reached. During the titration, the flask was been swirl. The end point was indicated when the entire solution retain a faint pink color for at least 30 seconds. The final burette reading was recorded. This was the result of the rough titration
5) The process were repeated until two consecutive titrations
INTRODUCTION
Reaction of acid and base is one of the most common reaction in chemistry. This reaction is also widely known as neutralization. In this experiment, we used titration technique which involves accurately measuring the volume of a solution required to react with another reagent. An indicator must be used to determine the end point of the titration. The indicator used can change colors at different pH values.
OBJECTIVE
To determine the concentration of sulphuric acid (H2SO4) using titration technique
CHEMICALS
NaOH solution, approximately 0.2 M, dilute sulphuric acid of unknown molarity, phenolphthalein
APPARATUS
Burette. Burette clamp, retort stand, 20 mL volumetric pipette, pipette filter, 250 mL conical flask
PROCEDURES
1) The burette was washed with distilled water and then rinsed with about 5-10 mL of NaOH solution, running the second rinsing through the burette tip. The burette was clamped to the retort stand
2) The burette was filled with the base, made sure the tip was completely filled and contain no air bubbles. The initial burette reading was recorded
3) Using a volumetric pipette, 20.00 mL H2SO4 was transferred to a clean 250 mL conical flask. 2 or 3 drops of phenolphthalein indicator was added. This flask was placed on a piece of white paper under the burette and the burette tip was lowered into the flask. The initial burette reading was recorded, to 2 decimal places
4) The acid was titrated by adding base until the end point was reached. During the titration, the flask was been swirl. The end point was indicated when the entire solution retain a faint pink color for at least 30 seconds. The final burette reading was recorded. This was the result of the rough titration
5) The process were repeated until two consecutive titrations