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(a) Explain why Mg(OH)2 precipitates when CO32– ion is added to a solution containing Mg2+. (b) Will Mg(OH)2 precipitate when 4.0 g of Na2CO3 is added to 1.00 L of a solution containing 125 ppm of Mg2+?
The pH of a 25 degree celcius groundwater containing 10-4M of Mg2+ is initially raised to 12. No further base is added. What will be the equilibrium pH and Mg2+ concentration? Assume that no carbonate species and no other ions are present that could precipitate and that Mg2+ precipitates as Mg(OH)2(s). Recall that for every one Mg2+ that precipitates, two OH- ions precipitate.
How many grams of Mg(OH)2 are required to obtain a 0.01M hydroxide solution.