Natural waters often contain relatively high levels of calcium ion, Ca²+, and hydrogen carbonate ion (bicarbonate), HCO3, from the leaching of minerals into the water. When such water is used commercially or in the home, heating of the water leads to the formation of solid calcium carbonate, CaCO3, which forms a deposit ("scale") on the interior of boilers, pipes, and other plumbing fixtures. Ca(HCO3)2(aq) → CaCO3(s) + CO₂(g) + H₂O(1) If a sample of well water contains 0.0016 mg of Ca(HCO3)2 per milliliter, what mass of CaCO3 scale would 1.0 mL of this water be capable of depositing?

Natural waters often contain relatively high levels of calcium ion, Ca²+, and hydrogen carbonate ion (bicarbonate), HCO3, from the leaching of minerals into the water. When such water is used commercially or in the home, heating of the water leads to the formation of solid calcium carbonate, CaCO3, which forms a deposit ("scale") on the interior of boilers, pipes, and other plumbing fixtures. Ca(HCO3)2(aq) → CaCO3(s) + CO₂(g) + H₂O(1) If a sample of well water contains 0.0016 mg of Ca(HCO3)2 per milliliter, what mass of CaCO3 scale would 1.0 mL of this water be capable of depositing?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Subject: chemistry
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