Standardization of Sodium Hydroxide Solution

Objectives

The objectives of this experiment are:

1. To standardize sodium hydroxide solution with potassium hydrogen phthalate using phenolphthalein as an indicator.
2. To determine the molarity or concentration of the standardized solution.
3. To calculate the concentration of the molarity based on the recorded experimental data.
4. To gain proficiency in executing titration techniques.
5. To observe the stages of titration and identify the endpoint using the color change of the analyte.

Materials

Table 1: Quantity of reagents for each solution

Table 2: Specification and quantity of laboratory apparatuses

Methodology

Preparation of Potassium Hydrogen Phthalate (KHP) Solution

1. Rinse four Erlenmeyer flasks to be used in titration.
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2. Weigh 0.5 g of KHP using a digital balance and transfer it to each flask.
3. Pipette 40 ml of water into a beaker and transfer it to each flask containing KHP.
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   Dissolve KHP thoroughly.

4. Add three drops of phenolphthalein to each flask, mix, and set aside.
5. Repeat steps 1-4 for the remaining flasks.

Preparation of Sodium Hydroxide (NaOH) Solution

1. Pipette 150 ml of sodium hydroxide and transfer it to an Erlenmeyer flask.
2. Close the flask with a stopper to prevent air/environmental reaction.

Preparation of Burette

1. Rinse the burette with distilled water. For the final rinse, use 3 ml of NaOH solution and drain it through the stopcock.
2. Attach the burette to a burette clamp mounted on a ring stand.
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3. Fill the burette with NaOH solution above the zero mark using a funnel. Open the stopcock to allow excess solution to reach the zero mark.
4. Ensure the burette tip is filled with solution and free of bubbles for accuracy.

Titration Set-up

Standardization of NaOH Solution

1. Position the Erlenmeyer flask containing KHP solution under the burette tip.
2. Place a white tile under the flask for color change detection.
3. Record the initial NaOH solution reading in the burette.
4. Titrate the first sample of KHP solution by slowly adding NaOH with constant swirling.
5. Observe the appearance of a faint pink color that persists for at least 30 seconds.
6. Record the final burette reading.
7. Calculate the estimated volume of titrant needed for subsequent titrations.
8. Titrate the remaining samples using the calculated volume with constant swirling until the endpoint is reached.
9. Record the final burette readings for each sample.

Calculation

1. Calculate the moles and molarity of the analyte using the recorded data.
2. Determine the molarity or concentration of the NaOH solution.
3. Repeat calculations for each sample.

Conclusion

The standardization of sodium hydroxide solution with potassium hydrogen phthalate using phenolphthalein indicator is a crucial procedure in analytical chemistry. By accurately determining the concentration of NaOH solution, it ensures precise results in subsequent experiments involving acid-base reactions. Through meticulous titration techniques and careful observation of endpoint indicators, analysts can reliably determine the molarity of solutions, facilitating various chemical analyses.