A solution contains 1.77 g of dissolved silver. How many moles of potassium chloride must be added to the solution to completely precipitate all of the silver? What mass of potassium chloride must be added?
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1 Answer
May 22, 2016
We need to add over
Explanation:
Clearly we need an equivalent quantity of chloride, thus we add a mass of potassium chloride:
Of course addition of the 1 equiv will precipitate most of the silver ion. Silver chloride will possess some (low) aqueous solubility, according to its solubility product. The result is a curdy white precipitate of silver chloride, that will be very hard to handle.
