Write a laboratory report on standardization of NaHCO3 using a 10ml graduate cylinder measure 10.0 ml of the acid solution and transfer the solution to a 125ml Erlenmeyer flask. Add 2-3 drop of phenolphthalein and titrate to the end point (light pink) with a standardized sodium hydrogen carbonate solution.
Title: Standardization of Sodium Hydrogen Carbonate (NaHCO3) using a 10 mL Graduate Cylinder and Phenolphthalein Indicator
Introduction:
The purpose of this laboratory experiment was to standardize a sodium hydrogen carbonate (NaHCO3) solution using a 10 mL graduate cylinder and phenolphthalein indicator. The sodium hydrogen carbonate solution was titrated against an acid solution to determine the exact concentration of NaHCO3.
Materials:
- Sodium hydrogen carbonate (NaHCO3) solution
- Acid solution
- 10 mL graduate cylinder
- 125 mL Erlenmeyer flask
- Phenolphthalein indicator
- Standardized sodium hydrogen carbonate solution
- Burette
- Distilled water
- Pipette
- Clamp
Procedure:
1. Using a 10 mL graduate cylinder, measure and transfer 10.0 mL of the acid solution to a clean 125 mL Erlenmeyer flask.
2. To the acid solution in the Erlenmeyer flask, add 2-3 drops of phenolphthalein indicator.
3. Prepare the standardized sodium hydrogen carbonate solution by dissolving an appropriate amount of NaHCO3 in distilled water.
4. Set up the burette and pour the standardized sodium hydrogen carbonate solution into the burette.
5. Record the initial burette reading.
6. Start titrating the acid solution in the Erlenmeyer flask by slowly adding the standardized NaHCO3 solution from the burette while swirling the flask.
7. Continue adding the NaHCO3 solution dropwise until a faint light pink color persists for approximately 30 seconds, indicating the end point.
8. Record the final burette reading.
9. Repeat the titration process thrice to obtain an average titre.
Results:
Initial burette reading: ________ mL
Final burette reading: ________ mL
Titrant Volume (mL)
Trial 1: ________ mL
Trial 2: ________ mL
Trial 3: ________ mL
Average: ________ mL
Calculations:
1. Calculate the volume of standardized NaHCO3 solution used in each trial by subtracting the initial burette reading from the final burette reading. Record the values in the table above.
2. Calculate the average volume of NaHCO3 solution used by summing up the volumes from each trial and dividing by the number of trials.
Discussion and Analysis:
The purpose of titrating the acid solution with the standardized NaHCO3 solution was to determine the concentration of the NaHCO3 solution. The phenolphthalein indicator was used to indicate the end point of the titration, which was observed as a faint light pink color persisting for approximately 30 seconds.
The average volume of the standardized NaHCO3 solution required to reach the end point was calculated as ________ mL. This value will be used in subsequent calculations to determine the concentration of the NaHCO3 solution.
Conclusion:
In this laboratory experiment, the sodium hydrogen carbonate (NaHCO3) solution was standardized using a 10 mL graduate cylinder and phenolphthalein indicator. The average volume of the standardized NaHCO3 solution required to reach the end point was determined as ________ mL. This information can be used to calculate the concentration of the NaHCO3 solution.