Magnesium ions can be precipitated from seawater by the addition of sodium hydroxide. How much sodium hydroxide in grams must be added to a sample of seawater to completely precipitate the 88.4 mg of magnesium present?
Step 1 of 3
Here, we have to determine the amount of sodium hydroxide required to precipitate all of the Mg.
Mg2+(aq) +2 NaOH(aq) ------> Mg(OH)2 (s) + 2Na+(aq)
Molar mass of NaOH =39.997 g/mol
Molar mass of Mg =24.305 g/mol
Thus,the conversion factors
g NaOH(aq)= mol NaOH(aq) = g Mg = mol Mg
Thus the amount of sodium hydroxide required
= 88.4 mg of Mg x x x x
= = 0.2909 g NaOH = 290.94 mg of NaOH
Therefore, 0.2909 g NaOH (290.94 mg of NaOH) is required to precipitate all the Magnesium ion from the reaction.
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
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