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Acid base titration
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Purpose:Ttrate and determine the molar concentration of a weak monoprotic acid using a strong base of
known volume and concentration.
Materials:
- 100 ml of unknown acid
- 5 ml of phenolphthalein indicator solution
- 3 mole/100 ml of sodium hydroxide
- 50 ml burette
- 2 Erlenmeyer flasks
Procedure:
1) “File” in the upper left corner was selected to open the assignment. “Load an assignment”
was chosen from the drop down list.
2) “Acids and bases were selected from the assignment list. “Unknown acid and base
problem” was selected after scrolling down and the arrow to the right of the title was
selected. The lab was opened.
3) There are 3 tabs in the stockroom, solutions, glassware and tools. The solutions tab was
selected. Unknown acid 0.1 L was selected from the list of solutions. This placed 100.00
ml of the unknown acid in an erlenmeyer flask on the lab workbench. Return to the
stockroom.
4) Indicators were selected from the solutions list. Phenolphthalein indicator solution was
chosen from the list. The indicator will turn pink when you have passed the end point.
5) The bottle of phenolphthalein was selected, held, moved over the top of the flask which
contained the unknown acid. A measurement box appeared. 5.00 ml of indicator solution
was added to the flask which contained the unknown acid. The indicator bottle was right
clicked and remove was chosen to take it from the workbench. Return to the stockroom.
6) A strong base was chosen from the list of solutions in the solution list. The type of base,
volume and molar concentration was noted. Return to the stockroom.
7) Other was selected from the glassware list. The 50.00 ml burette was chosen from the
drop down list. It was placed on the lab work bench.
8) The flask containing the base was selected, held, moved over the top of the burette. A
measurement box appeared. 50.00 ml of the base was added to the burette. The initial
burette reading was recorded.
9) The burette containing the base was selected, held, moved over the top of the flask which
contained the unknown acid. A measurement box appeared. The base was added to the
unknown acid at 5.00 ml increments (the pH readings in the panel at the left was
watched). Each increment of base added to the unknown acid along with corresponding
ph was recorded. As the color change was approached, the amount of base added was
reduced to 1.00 ml then 0.50 ml increments. Note: Smaller increments could be used to
get more precise results.
10) The endpoint was identified, the procedure was repeated past the endpoint. Se;ected
increments of the base were continuously added until the pH was approximately 11.
11) The concentration (molar concentration) of the unknown acid was calculated using the
data recorded.
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