You add potassium hydroxide to the solution in Example 18.13. When the [OH - ] reaches 1.9

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You add potassium hydroxide to the solution in Example 18.13. When the [OH-] reaches 1.9 * 10-6 M (as you just calculated), magnesium hydroxide begins to precipitate out of solution. As you continue to add KOH, the magnesium hydroxide continues to precipitate. However, at some point, the [OH-] becomes high enough to begin to precipitate the calcium ions as well. What is the concentration of Mg2+ when Ca2+ begins to precipitate?


Example 18.13

The magnesium and calcium ions present in seawater ([Mg2+] = 0.059 M and [Ca2+] = 0.011 M) can be separated by selective precipitation with KOH. What minimum [OH-] triggers the precipitation of the Mg2+ ion?

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