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CHM 121 Antacid Lab Report
- Course
- Chemistry 121
- Institution
- Harper College
This is a comprehensive and detailed lab report on; Antacid. *Essential!!
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Analysis of an AntacidBy: Jonathan Pilafas (performed on 10/15/2018)
Purpose: The objective of this lab is to compare different generic and name brand antacids to
determine if they are equally effective in neutralizing acid and if they are comparably cost
effective.
References:
1. “Laboratory Experiments for Chemistry 121” - Harper College
2. http://dept.harpercollege.edu/chemistry/msds1/Phenolphthalein%20JTBaker.pdf
3. http://dept.harpercollege.edu/chemistry/msds1/Hydrochloric%20acid%20Fisher.pdf
4. http://dept.harpercollege.edu/chemistry/msds1/Sodium%20hydroxide%20Fisher.pdf
5. http://dept.harpercollege.edu/chemistry/msds1/Calcium%20carbonate%20Fisher.pdf
Reagents:
Name Formula Molecular Concentration Hazards
Weight
Hydrochloric HCl 36.46 g/mol 36-38% Health - 3
Acid Fire - 0
Reactivity - 1
Sodium NaOH 40.00 g/mol 50% Health - 3
Hydroxide Fire - 0
Reactivity - 1
Phenolphthalein C20H14O4 318.312 g/mol N/A Health - 2
Fire - 1
Reactivity - 0
Tums CaCO3 Active Ingredient N/A Health - 2
in Antacid Fire - 0
Reactivity - 0
, Methods:
To begin the experiment, record the antacid brand name, the ingredients (active and
inactive) in your antacid, the mass of the active ingredient, the price of the bottle, and the
number of tablets in each bottle. Then, rinse the burets with deionized water and label them
accordingly. Next, obtain two antacid tablets and find the mass of each of these. After this,
obtain the HCl and NaOH solutions and record the molarities on the stock bottles. Next, put 15 -
25 mL of HCl solution into each of two clean Erlenmeyer flasks and record the exact volume of
HCl used in each Erlenmeyer flask.
Add one of the antacid tablets to each flask and heat gently for 1-2 minutes to help
dissolve the tablets. Bring each solution to a boil to get rid of any undissolved carbon dioxide.
After finishing this, allow the solution to cool. Once the solution is cool, add 2-3 drops of
phenolphthalein to antacid mixture. Lastly, titrate each antacid mixture with the NaOH solution
until you have reached the end point of the indicator used.
Balanced Chemical Equation:
- CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)
- NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)
Calculations:
- Moles HCl initial = (0.2500 L HCl / 1) X (0.9936 mol HCl / 1 L HCl) = 0.02484 mol HCl
initial
- Moles HCl excess = (0.01500L NaOH / 1) X (1.082 mol NaOH / 1 L NaOH) X (1 mol HCl
/ 1 mol NaOH) = 0.01623 mol HCl excess
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