If 50.0 mg of Na2CO3 are added to 150.0 mL of a solution that is 1.5 × 10−3 M in Mg2+, will any MgCO3 precipitate from the solution?
Solution 100P :
Molarity of tap water having Mg2+ = 1.5 × 10-3 M
Mass of Na2CO3 added = 50 mg.
Volume of solution = 150.0 mL
Will MgCO3 precipitate out of solution = ?
MgCO3 ionizes into :
MgCO3(S) Mg2+ (aq) + CO32- (aq)
We have the molarity of Mg2+. let’s calculate molarity of CO32- as :
Ksp = [Mg2+][CO32-]
Ksp of MgCO3 = 6.82 × 10-6
We are given the molarity of Mg2+, let’s substitute those values :
6.82 × 10-6 = 1.5 × 10-3 M [CO32-]
= 0.004546 M
This is the maximum soluble concentration of CO32- in the presence of 1.5 × 10-3 M Mg2+
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
The answer to “If 50.0 mg of Na2CO3 are added to 150.0 mL of a solution that is 1.5 × 10?3 M in Mg2+, will any MgCO3 precipitate from the solution?” is broken down into a number of easy to follow steps, and 28 words. Since the solution to 100P from 15 chapter was answered, more than 1448 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: solution, mgco, any, precipitate, added. This expansive textbook survival guide covers 19 chapters, and 2046 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 100P from chapter: 15 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.