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Follow the rate of an acid/base neutralization reaction between hydrochloric acid and calcium carbonate in a commercial antacid. Students explore how changing the acid concentration affects the production of carbon dioxide. Materials are sufficient for 15 student pairs.
The acid-base neutralization in this lab simulates what happens when antacids are taken to alleviate indigestion. Students collect the carbon dioxide produced from the reaction, using the water displacement method. Through graphical analysis of the volume of gas collected over time, students determine the effect that changing the concentration of hydrochloric acid has on the reaction rate. Materials are sufficient for 15 student pairs. General lab equipment and labware (ring stands, clamps, beakers, graduated cylinders) are needed but not supplied.
|Rubber Stopper, 1-Hole||15||Included|
|1 M Hydrochloric Acid, 500 mL||1||Included|
|Commercial Antacid, Roll||5||Included|
|Air Line Tubing, 8 ft||2||Included|
|Test Tube, 20 x 150 mm||15||Included|
|Teacher's Manual with Reproducible Student Guide||1||Included|
|Graduated Cylinder, 100 mL||15||Needed, Not Included|
|Ring Stand||15||Needed, Not Included|
|Clamp, Universal||15||Needed, Not Included|
|Test Tube Rack||15||Needed, Not Included|
|Beaker, 250 mL||15||Needed, Not Included|
|Timing Devices||15||Needed, Not Included|
|Paper Towels||Needed, Not Included|
|Water||Needed, Not Included|