THE TITRATION CHALLENGE – Battle of the Burets!!
(Lab Guidelines: 1,2,3,4,5,6,7,9,10,11,12)
Purpose:
To use titration to determine the concentration of a solution of hydrochloric acid using a solution of 0.600 M
sodium hydroxide.
Introduction:
What is a titration?
Using a ______________________ of known ___________________________to determine the _________________________ of some
other _______________________. Titrations are most commonly used to determine the concentrations of various
_______________ and ______________.
What is the titrant? The titrant is the __________________________ of known _______________________________.
Equipment and Materials:
Ring stand, buret clamp, 50 mL buret, buret funnel, 250mL beaker for sample, 600mL beaker for waste, glass
rod, 50 mL graduated cylinder, phenolphthalein indicator, 0.600 M NaOH, ??MHCl
Procedure:
Design a procedure to determine the concentration of the hydrochloric acid solution. You must write a
bulleted procedure, and underline all the materials in your procedure. Here are a few guidelines:
1. Use 50.0 mL of HCl (add about 5 drops of phenolphthalein).
2. Add NaOH carefully. Stir Frequently.
3. How will you know when you are finished with the titration?
4. Do two trials. Record data for both, but only use data from the best trial to do calculations.
Note: the best trial should be the second trial. The first trial is a “scrap” trial.
Data:
Keep track of the volume of titrant used to reach the end of the reaction for each trial.
Calculations:
First write the balanced equation for the reaction which took place in the beaker.
Show all necessary calculations to determine the concentration of the HCl. Keep in mind that this is just a
new type of stoichiometry problem. You should use only the titration which you felt was completed most
masterfully. Ignore any other data.
Question:
50.0 mL of HCl is titrated with a solution of barium hydroxide. If it requires 33.4 mL of 0.100 M barium
hydroxide to reach the endpoint of the titration, then calculate the concentration of the HCl solution. (You
must write the balanced equation first!)
Error Analysis:
Calculate your percent error for the concentration of the HCl and discuss possible sources of error.
Conclusion:
Write a conclusion which demonstrates that you understand what you did. How did you accomplish the
purposes? Discuss the math as well.
Remember, here is a great guide for writing your conclusion:
1) Restate the purpose
2) Summarize the procedure and data collection
3) Discuss any important principles / equations used
4) Explain the graphs and/or math
5) Report your results
Also, please include any other interesting information you would like to add.