Water containing Ca2+ and Mg2+ ions is called hard water and is unsuitable for some household and industrial use because these ions react with soap to form insoluble salts, or curds. One way to remove the Ca2+ ions from hard water is by adding washing soda (Na2CO3 • 10H2O). (a) The molar solubility of CaCO3 is 9.3 × 10−5 M. What is its molar solubility in a 0.050 M Na2CO3 solution? (b) Why are Mg2+ ions not removed by this procedure? (c) The Mg2+ ions are removed as Mg(OH)2 by adding slaked lime [Ca(OH)2] to the water to produce a saturated solution. Calculate the pH of a saturated Ca(OH)2 solution. (d) What is the concentration of Mg2+ ions at this pH? (e) In general, which ion (Ca2+ or Mg2+) would you remove first? Why?
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