PLEASE NOTE: Titration requires several steps in order to obtain exact results. The procedures described in this lab assume that you have already done the TITRATION TUTORIAL and are familiar with the technique.
1. Prepare the NaOH solution by dissolving approximately 4g of solid NaOH in 200 mL of water in a 250 ml beaker. Calculate the approximate NaOH concentration:
a. Convert grams of NaOH to moles of NaOH (MW = 40.00, moles = g/MW)
b. Calculate Concentration of NaOH (Molarity = moles/Liter, Remember: 1 Liter = 1000mL) Record this amount.
2. To prepare the primary standard, first calculate and record the expected mass of benzoic acid required to react in stoichiometric proportion with 20 mL of the NaOH solution:
a. From the balanced acid-base reaction,
C7H6O2 + NaOH -> NaC7H5O2 + H2O, you know that the acid to base ratio is 1:1
b. Find moles of NaOH (moles = Molarity x Volume(L))
c. Convert moles of NaOH to moles of C7H6O2 using ratio of 1:1
d. Convert moles of C7H6O2 to grams of C7H6O2. (grams = moles x Molecular Weight, MW = 122.12) Record this mass.
3. Add the calculated mass of benzoic acid to a clean Erlenmeyer flask and dissolve in 50 mL of water. Add 2 drops of phenolphthalein.
4. Fill a 50 mL burette with NaOH and record the initial volume.
5. Connect the Erlenmeyer flask containing the benzoic acid solution to the base of the burette stand. Open the Data window and click the Pushpin icon to keep the data display set to the flask.
6. Titrate the benzoic acid solution by adding NaOH solution in large increments at first and then in small increments. Open the Properties window and click on the buret. Enter the amount of titrate to add, and click either the drop or flow buttons to deliver the desired amount.
7. Once the solution in the Erlenmeyer flask turns pink, you have reached - and probably passed - the endpoint of the titration.
8. Repeat the analysis with another flask of
benzoic acid solution prepared EXACTLY as before. Refill the burette with NaOH solution. This time, add NaOH in large increments until you get NEAR the endpoint of the previous trial.
9. Change to adding drops instead of mL, and add NaOH solution until the endpoint is reached as exactly as possible. You should be able to determine the endpoint to within 0.02 mL.
10. With the total volume of NaOH solution used to titrate the benzoic acid primary standard, calculate the concentration of the NaOH solution.
11. Repeat the precise titration twice more and compare the 3 NaOH concentrations. They should be within 1% of each other.
12. The rest of the NaOH solution can now be used in further lab work as a secondary standard with a reliably known concentration equal to the average of the 3 titrations.
Procedure 2 ( click to view assignments for this procedure )
Acetic Acid of Unknown Concentration
1. In an Erlenmeyer flask, add 25 mL of acetic acid of unknown concentration and 2 drops of phenolphthalein indicator.
2. Refill the burette with the NaOH solution (standardized in Procedure 1), and record the initial volume.
3. Titrate the acetic acid sample to the phenolphthalein's color change endpoint. Record the final volume of the NaOH in the buret. Calculate the concentration of the acid.
4. Repeat the titration 2 more times and calculate the acid concentration of each trial.
5. Give the final acid concentration as the average of the 3 results.
and List all measurements and include proper labels.
Molecular weight of benzoic acid: 122.12 g/mole
Mass of benzoic acid used:
Titration of NaOH and benzoic acid: (Fine Titrations Only)
Trial 1 Trial 2
Initial volume(NaOH)(ml)
final volume(NaOH)(ml)
Calculations/Interpretations:
Show all math performed (label the calculation or give the formula, show your setup, and give the result) and include proper labels. Also, answer any questions asked in the lab.
Moles of Benzoic acid:
Moles of NaOH:
Trial 1 Trial 2
Volume of NaOH used (ml):
Volume of NaOH (L):
Molarity of NaOH:
(Enter Assignment Report)
Assignment 1 of Procedure 2
Data: List all measurements and include proper labels.
Volume of acetic acid (ml):
Titration of NaOH and acetic acid: (Fine Titrations Only)
T1 T2
Initial volume(NaOH)(ml)
final volume(NaOH)(ml)
Calculations/Interpretations:
Show all math performed (label the calculation or give the formula, show your setup, and give the result) and include proper labels. Also, answer any questions asked in the lab.
Trial 1 Trial 2
Volume of NaOH used (ml)
Volume of NaOH (L):
Moles of NaOH (molarity times volume):
Moles of Aceitc Acid:
Volume of Acetic Acid (L):
Molarity of Acetic Acid:
To perform a titration and calculate the concentrations of NaOH and acetic acid, follow these steps:
Procedure 1: NaOH Solution
1. Prepare the NaOH solution by dissolving approximately 4g of solid NaOH in 200 mL of water in a 250 ml beaker. To calculate the approximate NaOH concentration:
a. Convert grams of NaOH to moles of NaOH using the molecular weight (MW = 40.00, moles = g/MW).
b. Calculate the concentration of NaOH in moles per liter (Molarity = moles/Liter). Remember that 1 liter is equal to 1000 mL. Record this value.
2. To prepare the primary standard, calculate and record the expected mass of benzoic acid required to react with 20 mL of the NaOH solution in stoichiometric proportion:
a. From the balanced acid-base reaction, C7H6O2 + NaOH -> NaC7H5O2 + H2O, we know the acid to base ratio is 1:1.
b. Find moles of NaOH by multiplying the molarity by the volume in liters (moles = Molarity x Volume).
c. Convert moles of NaOH to moles of C7H6O2 using the 1:1 ratio between the acid and base.
d. Convert moles of C7H6O2 to grams of C7H6O2 using the molecular weight (grams = moles x Molecular Weight, MW = 122.12). Record this mass.
3. Add the calculated mass of benzoic acid to a clean Erlenmeyer flask and dissolve in 50 mL of water. Add 2 drops of phenolphthalein.
4. Fill a 50 mL burette with NaOH solution and record the initial volume.
5. Connect the Erlenmeyer flask containing the benzoic acid solution to the base of the burette stand. Open the Data window and click the Pushpin icon to keep the data display set to the flask.
6. Titrate the benzoic acid solution by adding NaOH solution in large increments at first, and then in small increments. Open the Properties window and click on the burette. Enter the amount of titrate to add, and click either the drop or flow button to deliver the desired amount.
7. Once the solution in the Erlenmeyer flask turns pink, you have reached - and probably passed - the endpoint of the titration.
8. Repeat the analysis with another flask of benzoic acid solution prepared exactly as before. Refill the burette with NaOH solution. This time, add NaOH in large increments until you get near the endpoint of the previous trial.
9. Change to adding drops instead of mL, and add NaOH solution until the endpoint is reached as exactly as possible. You should be able to determine the endpoint to within 0.02 mL.
10. With the total volume of NaOH solution used to titrate the benzoic acid primary standard, calculate the concentration of the NaOH solution.
11. Repeat the precise titration twice more and compare the 3 NaOH concentrations. They should be within 1% of each other.
12. The rest of the NaOH solution can now be used in further lab work as a secondary standard with a reliably known concentration equal to the average of the 3 titrations.
Procedure 2: Acetic Acid of Unknown Concentration
1. In an Erlenmeyer flask, add 25 mL of acetic acid of unknown concentration and 2 drops of phenolphthalein indicator.
2. Refill the burette with the NaOH solution standardized in Procedure 1, and record the initial volume.
3. Titrate the acetic acid sample until you reach the phenolphthalein's color change endpoint. Record the final volume of the NaOH in the burette.
4. Repeat the titration two more times and calculate the acid concentration for each trial.
5. Give the final acid concentration as the average of the three results.
By following these steps, you can carry out a titration and calculate the concentrations of NaOH and acetic acid.