Procedure I. Carbonate in the Limestone 1. Using a hammer (or other heavy object

Question

Procedure I. Carbonate in the Limestone 1. Using a hammer (or other heavy object, break a piece of limestone into small pieces ideally, the pieces should have masses no greater than each. 2. Select one (or a few) pieces of limestone that have a total mass of g; record the mass s m L3. Add approximate of 3.00 M HCl to a clean and dry (important!) 125-mL Erlenmeyer flask. Record the total mass of the container with the HC1 4. Add the limestone to the flask with the HC the limestone should begin to dissolve with the formation of bubbles (production of CO2 gas). Allow the reaction to proceed until the mixture stops bubbling/foaming, indicating that the reaction is complete. 5. Record the final mass of the container remaining contents. Do not dispose of the solution-you will continue using this mixture for Part II 6. Repeat steps 1 to 5. This will give you two sets of data for Part I, and two samples to move forward to Part II II. Calcium in the Limestone gravity hltruhan For each sample from Part I solid 7. The limestone sample in Part I should have completely dissolved in the HCl solution. did not dissolve (impurities such as silicates, sulfides, and sulfates), one can carefull filter at this step and place the filtrate into a clean 125-mL Erlenmeyer flask for use in the rest of the tab s. Measure the mass of a clean and dry Gooch crucible together with a piece of filter paper placed inside the 76 Laboratory 7 Percent composition from Gravimetric Analysis: calcium Carbonate in Texas Limestone

Explanation / Answer

3) No, you cannot find the amount of CO2 lost because you need to find the amount of precipitate
   first and later obtain the amount of CO2
4) Try filtering, if there is any leftover wet solvent it will pass through filtrate, if it is dry you can just
observe dry solid without any solvent .

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