An Introduction To Titration Lab Report
An Introduction to Titration: Standardization of HCl and NaOH Lab Report
Introduction:
It is important to standardize solutions in order to have the accurate amount of concentration known. A standard solution can be prepared in either of two ways: A primary standard is carefully weighed, dissolved, and diluted accurately to a known volume. Its concentration can be calculated from this data. A solution is made to an approximate concentration and then standardized by titrating an accurately weighed quantity of a primary standard. Solid NaOH has the property of absorbing water from the air so it is not possible to accurately weigh NaOH. Sodium hydroxide is unsuitable as a primary standard because of this property. You must use method two for preparing a standard solution, using oxalic acid dehydrate. The expected chemical reactions are listed below.
Chemical Reactions:
a.) HCl and Na2CO3 = 2NaCl + CO2 + H2O
b.) KHP and NaOH = KNaP + H2O
Experimental Procedure:
1. Get an Erlenmeyer flask (250 mL) and add 100 mL of distilled water to it.
2. Weigh .15 of NaCO2 and add it to the distilled H2O.
3. Now add .5-1 mL of bromocresol to the flask.
4. Fill up the buret with HCl
5. Let the buret drip into the flask until the color turns green then stop buret.
6. Once it is a green color place it on a burner to boil it, add stir bar so it keeps the solution moving.
7. Leave it on the burner until it turns blue again, once blue take off burner and let cool down.
8. Place flask under the buret and let HCl into the flask until the color turns yellow.
9. Read buret to get mL of HCl (.0029 L)
10. Get another Erlenmeyer flask (250 mL) and add 100 mL of distilled water.
11. Weigh .5 KHP and add it to the water, stir until dissolved. Add 4 drops of phenophitrolein.
12. Fill the buret with NaOH (100 mL)
13. Let the buret drip into the flask until the solution turns pink.
Results:
The molarity of the HCl and NaOH table ranged from 0.907-0.976, which showed neither accuracy nor
Introduction:
It is important to standardize solutions in order to have the accurate amount of concentration known. A standard solution can be prepared in either of two ways: A primary standard is carefully weighed, dissolved, and diluted accurately to a known volume. Its concentration can be calculated from this data. A solution is made to an approximate concentration and then standardized by titrating an accurately weighed quantity of a primary standard. Solid NaOH has the property of absorbing water from the air so it is not possible to accurately weigh NaOH. Sodium hydroxide is unsuitable as a primary standard because of this property. You must use method two for preparing a standard solution, using oxalic acid dehydrate. The expected chemical reactions are listed below.
Chemical Reactions:
a.) HCl and Na2CO3 = 2NaCl + CO2 + H2O
b.) KHP and NaOH = KNaP + H2O
Experimental Procedure:
1. Get an Erlenmeyer flask (250 mL) and add 100 mL of distilled water to it.
2. Weigh .15 of NaCO2 and add it to the distilled H2O.
3. Now add .5-1 mL of bromocresol to the flask.
4. Fill up the buret with HCl
5. Let the buret drip into the flask until the color turns green then stop buret.
6. Once it is a green color place it on a burner to boil it, add stir bar so it keeps the solution moving.
7. Leave it on the burner until it turns blue again, once blue take off burner and let cool down.
8. Place flask under the buret and let HCl into the flask until the color turns yellow.
9. Read buret to get mL of HCl (.0029 L)
10. Get another Erlenmeyer flask (250 mL) and add 100 mL of distilled water.
11. Weigh .5 KHP and add it to the water, stir until dissolved. Add 4 drops of phenophitrolein.
12. Fill the buret with NaOH (100 mL)
13. Let the buret drip into the flask until the solution turns pink.
Results:
The molarity of the HCl and NaOH table ranged from 0.907-0.976, which showed neither accuracy nor