A 214.0-mL aliquot of 0.360 M aqueous potassium hydroxide is mixed with 214.0 mL of 0.360 M aqueous magnesium nitrate. The balanced formula equation is: 2KOH(aq) + Mg(NO3)2(aq) -> Mg(OH)2(s) + 2KNO3(aq)The precipitate is magnesium hydroxide Mg(OH)2.The mass of precipitate produced is 2.25g Calculate the concentration of each ion remaining in solution after precipitation is complete. Assume that the precipitate is completely insoluble.Concentration of K+ =____M Concentration of OH- =____M Concentration of Mg2+ =____M Concentration of NO3- =____M
A 214.0-mL aliquot of 0.360 M aqueous potassium hydroxide is mixed with 214.0 mL of 0.360 M aqueous magnesium nitrate. The balanced formula equation is: 2KOH(aq) + Mg(NO3)2(aq) -> Mg(OH)2(s) + 2KNO3(aq)The precipitate is magnesium hydroxide Mg(OH)2.The mass of precipitate produced is 2.25g Calculate the concentration of each ion remaining in solution after precipitation is complete. Assume that the precipitate is completely insoluble.Concentration of K+ =____M Concentration of OH- =____M Concentration of Mg2+ =____M Concentration of NO3- =____M
General Chemistry - Standalone book (MindTap Course List)
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Chapter4: Chemical Reactions
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Problem 4.116QP: Bone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride,...
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A 214.0-mL aliquot of 0.360 M aqueous potassium hydroxide is mixed with 214.0 mL of 0.360 M aqueous magnesium nitrate.
The balanced formula equation is:
2KOH(aq) + Mg(NO3)2(aq) -> Mg(OH)2(s) + 2KNO3(aq)
The precipitate is magnesium hydroxide Mg(OH)2.
The mass of precipitate produced is 2.25g
Calculate the concentration of each ion remaining in solution after precipitation is complete. Assume that the precipitate is completely insoluble.
Concentration of K+ =____M
Concentration of OH- =____M
Concentration of Mg2+ =____M
Concentration of NO3- =____M
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