Environmental / Chemical Engineering Problem Help

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SUMMARY

The forum discussion centers on calculating the concentration of magnesium ions in a solution containing 0.001000 M hydroxyl ions at 25 degrees Celsius. The correct concentration is established as 0.1367 mg/L. To solve this problem, users are advised to reference the equilibrium constant for the dissociation of magnesium hydroxide in aqueous solution, which is essential for understanding the relationship between magnesium ions and hydroxyl ions in solution.

PREREQUISITES
  • Understanding of chemical equilibrium principles
  • Knowledge of magnesium hydroxide dissociation
  • Familiarity with molarity calculations
  • Basic skills in analytical chemistry
NEXT STEPS
  • Research the equilibrium constant for magnesium hydroxide dissociation
  • Study the concept of solubility product (Ksp) in aqueous solutions
  • Learn how to perform molarity calculations for ionic compounds
  • Explore the effects of temperature on solubility equilibria
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Students in environmental and chemical engineering, educators teaching analytical chemistry, and anyone involved in water quality analysis and ion concentration calculations.

ride5150
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I have a environmental engineering problem to do for homework, it goes like this:

How many mg/L of magnesium ion will remain in solution in water that is 0.001000 M in hydroxyl ion and at 25 degrees celsius?

the answer is 0.1367 mg/L, but i don't know how it was found.

to be honest I am not even sure where to begin, for some reason i can't find the section in my book that deals with problems like this. if anyone could point me in the right direction id greatly appreciate it, or maybe tell me what topic i should look under in my book.

thank you
 
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Look up the equilibrium constant for the dissociation of magnesium hydroxide in aqueous solution.
 

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