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) S CaCO3(s) _ CO2(g) _ H2O(l) If a sample of well water contains 2.0 _ 10_3 mg of Ca(HCO3)2 per milliliter, what mass of CaCO3 scale would 1.0 mL of this water be capable of depositing?
Electrolytes are very important in the functioning of our nervous system, muscles, and heart. Your body needs to have a certain level of the electrolytes – not too many, not too few Covalent Bonds 1. These bonds are created when atoms share electrons. They are “borrowed”. 2. The sharing of atoms creates bonds that are MUCH stronger than ionic bonds. 3. Many carbon-containing compounds form covalent bonds. Hydrogen also tends to form covalent bonds.