When KHP is added to the solution of NaOH and the indicator, the solution will turn clear and neutralize. The concentration of NaOH is going to be very low because it is diluted. Materials required: pipette filler, volumetric flasks(2-4), beakers(2),small white piece of paper, indicator( 2 drops), conical flask, clamp, soap, eye protection, burette, distilled water, cleaning utensils, stand, funnel, solutions( NaOH and KHP) Procedure: . Gathered all materials required 2. Wore proper safety equipment 3. All the equipment was washed and gathered. 4. The base (NaOH) and the acid (KHP) were labeled and put into conical flasks and beakers. 5. A rod was screwed into the hole which is in the desk. Also a clamp was placed on the rod. 7. The burette was placed on the clamp. 8. The funnel was rinsed with some acid (KHP) from the inside as well as the outside. 9. A very little amount of acid was poured into the burette to clean it and a beaker was placed underneath the burette. 0. The burette was opened from the bottom to let the acid fall out. 11. A funnel was placed on top of the burette, and a piece of paper was placed between the funnel and flask to let oxygen escape. 12. The acid was poured into the burette until it reached 2 or 3 mL. 13. The pipette was taken to the sink and was rinsed from the outside bottom of the pipette with NaOH. 14. A very little amount of NaOH was poured into the pipette and was disposed into the sink. 15.
The Term Paper on NaOH Standardization and Titration of an Unknown Organic Acid
NaOH Standardization and Titration of an Unknown Organic Acid Overview: Methods for counting the number of molecules in a sample is a major emphasis of laboratory work. In this experiment we will use the method of titration to count the number of acid molecules in a solution. Measuring mass is a relatively easy procedure to do in the lab (although a balance is expensive). Counting the number of ...
The pipette was put into the pipette filler and the roller at the side of the pipette filler was rolled up slowly so that the pipette got filled with NaOH 16. The pipette filler was taken off and a thumb was placed on top of the pipette so that NaOH didn’t fall from pipette. 17. The base from the pipette was emptied into the conical flask. 18. A small amount of base left over in the pipette was emptied into the conical flask by turning the pipette around . 19. 2 to 3 drops of indicator were poured into the conical flask which contained the base NaOH. 0. The conical flask of the solution containing NaOH and the indicator was placed under the burette. 21. The burette stopper at the bottom of the burette was opened to let the acid fall through. 22. When the NaOH solution changes colour an becomes clear, close the burette. 23. The volume of the titrated solution was recorded. 24. The titrated solution was disposed. 25. The materials used were washed with soap and put back where they belonged. Observations: 250 ml of NaOH and 0. 1M of KHP Trial 12 Final (vol/cm3) 39. 5 ml50 mL
Initial(vol. /cm3)30. 5mL39. 5 mL Volume Used (ml)9. 0 mL11. 5 mL Calculations: Average volume of KHP used : 9. 0 mL +11. 5 NaOH (aq) + KHC8H4O4 (aq) ———————– NaKC8H4O4 (aq) + H2O (l) 1 : 1 : 1 : 1 Average volume used: 9. 25 mL Concentration of KHP: 0. 1 mol/L Volume of NaOH: 50 mL Mole Ratio: NaOH + KHC8H4O4 (1 : 1) KHP = 9. 25 mL x 0. 1mol/1L = 0. 925 mmol Since mole ratio= 1 : 1 NaOH= 0. 925 mmol
NaOH = 0. 925 mmol x 1/1 = 0. 925 mmol 50 mL of NaOH= 0. 925 mmol 50ml Concentration of NaOH= Discussion: NaOH is the secondary standard, therefore it’s concentration varies with time and is unstable. KHP is the primary standard, therefore it’s concentration is consent and stable. This experiment was conducted to titrate NaOH with KHP. When the NaOH was titrated with KHP it produced a solution which was neutralized and therefore contained salt and water. This proves that when a base and acid is combined salt and water are produced.
The Term Paper on Aqueous Solution Acid Base Conjugate
CHEMISTRY 122 CHAPTER 17 NOTES CHAPTER 17 EXERCISES (THESE ARE NOT TO BE TURNED IN, BUT QUIZ QUESTIONS WILL BE TAKEN FROM THESE EXERCISES SO IT IS TO YOUR BENEFIT TO DO THEM): 2, 3, 5, 6, 8, 10, 13, 15, 16, 18, 19, 21, 23, 25, 27, 28, 29, 31, 33, 37, 39, 41, 43, 44, 47, 48, 50, 53, 57, 60, 63, 64, 67, 70, 71, 73, 75, 78, 80, 87, 95, 102, 112 Chemistry of Acids and BasesSvante Arrhenius (1884) ...
When the indicator was added to the base NaOH it turned pink but when the acid KHP was added to the solution of the indicator and NaOH, the solution became clear again. There were many safety precautions that we had for this titration. These precautions included: – A paper was placed between the flask and the funnel so that oxygen escaped and to avoid spills. – All of the equipment was cleaned and washed properly so that there weren’t any extra materials or liquids in the experiment. – The burette was placed straight on the clamp and was secured so that it wouldn’t fall. The base was put in the pipette and not in the burette because the burette would have corroded. – Water was poured on sides of the conical flasks to avoid spills There were also sources of error we had for this experiment. These errors could have been avoided and in the future they will be. These errors included: -the amount of KHP finished fast and we were only able to do 2 trials – Were not wearing goggles at all times -we should have been more focused while conducting the experiment
Conclusion: In conclusion, overall the experiment went well. The design, materials and skills used in this experiment were sufficient because this lab produced the type of evidence needed to answer the question with a high degree of certainty. The steps were simple and easy to follow. My prediction was also correct because the concentration of NaOH was very low. The result was a base successfully titrated with an acid. The molar concentration of NaOH was successfully achieved by titrating NaOH with a standardized solution of KHP.
