How to Dissolve Calcium Oxalate

Unlike many other calcium compounds, calcium oxalate is insoluble in water.
••• abstract ripples image by Alexey Klementiev from Fotolia.com

Calcium oxalate is an ionic compound with the chemical formula CaC2O4 and a salt of oxalic acid. It's highly insoluble and dissolves poorly in water. One method for dissolving calcium oxalate in the lab is the application of a compound called ethylenediaminetetraacetic acid or EDTA. EDTA is highly effective at binding the calcium ions and thereby decreasing the concentration of calcium in solution, shifting the reaction equilibrium so that more calcium oxalate will dissolve. In the procedure outlined below, you'll first make calcium oxalate using common chemicals then dissolve it using EDTA.

    Put on the goggles and gloves. Oxalic acid and calcium oxalate are potentially toxic if ingested. Perform this experiment under the fume hood for safety.

    Measure out .032 ounces (.9 grams or approximately .01 moles) of oxalic acid into the beaker and add just under .338 fluid ounces (10 milliliters) of water. Swirl it gently in the beaker until the oxalic acid dissolves.

    Add .049 ounces (roughly 1.3 grams) of calcium chloride to the solution and swirl gently. As the reaction progresses, solid calcium oxalate will form and precipitate out of the solution. You now have calcium oxalate--the same substance from which kidney stones often form.

    Add about .01 ounces (.29 grams) of EDTA to the solution and swirl it gently in the beaker. Some of the calcium oxalate should begin to dissolve.

    Things You'll Need

    • EDTA (available from some science supply stores)
    • Calcium chloride (available at some automotive and hardware supply stores)
    • Oxalic acid (available from many hardware stores)
    • Water
    • Fume hood
    • Safety goggles
    • Gloves
    • Beaker
    • Measuring scale

    Tips

    • Dissolving calcium oxalate with EDTA is an application of Le Chatelier's principle. When calcium oxalate dissolves, it dissociates into calcium ions and oxalate ions. By binding the calcium ions with the EDTA, we reduce the concentration of the products, so we shift the process to the right even though the equilibrium constant does not change. Other substances that bind or react with the oxalate ions or the calcium ions should have the same effect as well.

    Warnings

    • Calcium oxalate and oxalic acid are hazardous if ingested or allowed to come in contact with eyes or skin. Never perform this experiment without gloves, safety goggles and proper safety equipment. Never eat or drink preparations of oxalic acid or calcium oxalate. Never ingest EDTA or bring it in contact with your eyes or skin except as directed by a physician.

Related Articles

How to Test for Calcium Hydroxide
How to Dissolve EDTA in Water
How to Make Magnesium Chloride
How to Make Sodium Nitrate
How to Extract Iodine From Potassium Iodide
How to Make Homemade Glow Sticks
How to Calculate w/v (Weight by Volume)
How to Do Titration Calculations
How to Calculate Solubilities
How to Reduce Potassium Permanganate
How to Calculate Molar Mass
How to Dissolve Calcium Chloride
How to Make Acetate From Vinegar
How to Dissolve Sodium Bicarbonate
How to Make an Ascorbic Acid Solution
How to Test for Sodium Bicarbonate
How to Make an EDTA Solution
Titration of Sodium Carbonate With Hydrochloric Acid
How to Calculate Particle Concentration
How to Dissolve Magnesium Chloride

Dont Go!

We Have More Great Sciencing Articles!