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when 100.0 mL of a 2.00 M solution of KOH(aq) is added to 100.0 mL of a 2.00 M solution of Mg(NO3)2 what is the mass of the precipitate(s) that form?

when 100.0 mL of a 2.00 M solution of KOH(aq) is added to 100.0 mL of a 2.00 M solution of Mg(NO3)2 what is the mass of the precipitate(s) that form?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 88QRT: You need to make a 0.300-M solution of NiSO4(aq). Calculate the mass of NiSO4 · 6H2O you should put...
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when 100.0 mL of a 2.00 M solution of KOH(aq) is added to 100.0 mL of
a 2.00 M solution of Mg(NO3)2 what is the mass of the precipitate(s) that form?









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how did the mass go from 58.3g to 5.83g?

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What is the concentration in molarity of the cations that remain in solution?

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