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Standarisation of Sodium Hydroxide Solution

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Introduction

Standarisation of Sodium Hydroxide Solution Aim: To investigate the concentration of Sodium Hydroxide. Identification of Variables: Dependent variable: * The volume of Hydrochloric acid used in titration. Independent variable: * The concentration of Sodium Hydroxide used in the experiment. Controlled variables: * The volume of Sodium Hydroxide used in titration process * The concentration of Hydrochloric acid. Materials required: o 0.1 mol dm-3 Hydrochloric acid solution o Sodium Hydroxide solution o Phenolphthalein o 50 mL Burette o 25 mL pipette o Dropping pipettes o 10 mL beaker glass o 100 mL conical glasses o Clamp stand Procedure: 1. Using the appropriate technique pipette 25 mL of NaOH solution into a 100 mL conical flask. 2. Add 1 drop of phenolphthalein to the NaOH solution. 3. Pour approximately 35 mL of 0.1 mol dm-3 HCl to the burette. 4. Place the NaOH solution below burette. ...read more.

Middle

NaOH = No of mol of HCl titrated Concentration of NaOH = No of mol of NaOH / volume of NaOH Average of volume of HCl titrated [mL] (� 0.2 mL) 9.15 No of mol of HCl titrated [mol] (� 2%) 0.000915 No of mol of NaOH [mol] (� 2%) 0.000915 Concentration of NaOH [mol dm-3 ] (� 2%) 0.0366 Evaluation of Experimental Procedure: The estimated systematic error could occur when I did the 1st experiment, as the result was not close to the other two results. This is related to the rapid titration that I did to find the rough estimate. The result became not accurate. The main concern is the used of secondary standard. HCl has small Mr, therefore in calculation process; the percentage of error would be larger. It means that the error could increase. I could decrease the error by using primary standard, which are KHP or Na2O3 . ...read more.

Conclusion

Because everybody has their own opinion whether the solution is colorless enough or not. Perhaps I made a wrong decision when I stopped the titration - whether it was too early or too late - therefore it would be better if I used digital pH meter. I could stop the titration when the digital pH meter showed that the pH was 7 - which is neutral- and it would decrease the error. Moreover, digital pH meter has an exact uncertainty; therefore the result would be even more accurate. From my experience in the 1st titration, I should shake the NaOH solution gently when I was doing titration. It made the solution mixed quickly, and it would reduce the error. I think another sources of error were small, as the apparatus used to measure the solutions have relatively small uncertainties such as burette (0.05 mL) and pipette (0.1 mL), and I followed the rest of the procedure correctly. Conclusion: The concentration of the NaOH solution used in this experiment is approximately 0.0366 �2% mol dm-3. ?? ?? ?? ?? ...read more.

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