These supplies are needed: distilled water
0.1 M HCl (8.3 mL concentrated HCl per 1 L of solution)
CAUTION: WEAR GOGGLES! HANDLE CONCENTRATED ACIDS UNDER ADULT SUPERVISION IN AN AREA WITH ADEQUATE VENTILATION. ALWAYS ADD ACID TO THE PRE-MEASURED WATER.
0.001 M HCl (1 mL 0.1 M HCl per 100 mL of solution)
0.00001 M HCl (1 mL 0.001 M HCl per 100 mL of solution)
marble, limestone, or chalk chips
pipette (glass with suction bulb or disposable)
4 test tubes
goggles
Follow these directions and complete the activities.

Set up four test tubes in a rack.
Add a small marble chip to each of the test tubes.
Add 1 mL samples of acid solutions as labeled in the chart.
Start with the weakest solution (distilled water) and work your way up in concentration. In this manner, you may use a single pipette for the entire experiment. Each test solution will simply increase the density of ions added to the chalk. Can you understand why you cannot return to a weaker solution with the same pipette?
Observe whether reaction takes place and how fast. Record your results.
Pour the acid solution from each test tube into the sink.
Rinse the marble chips with water and place them in a container for this purpose to be used again.
Observations:

Data Table:

distilled water 0.0001M HCl 0.001 M HCl 0.1 M HCl
strength of reaction
speed of reaction
Analysis:

Marble is made from limestone under the influence of heat and pressure. The chemical formula for limestone or marble chips is CaCO3. When you added the chips to the acid solutions, they effervesced (bubble or foam).

What is the gas that is produced?
What is the chemical formula of the gas?
How could you test rocks for the presence of limestone?
Write a balanced symbol model for the reaction of limestone with hydrochloric acid.