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...
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
Since the solution to 86P from 8 chapter was answered, more than 1143 students have viewed the full step-by-step answer. The answer to “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?” is broken down into a number of easy to follow steps, and 36 words. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. This full solution covers the following key subjects: sodium, seawater, magnesium, hydroxide, much. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. The full step-by-step solution to problem: 86P from chapter: 8 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.