What is the Magnesium Activity in Springs Near Jenner with a pH of 9.5?

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SUMMARY

The discussion centers on calculating the magnesium ion concentration in springs near Jenner with a pH of 9.5. The equilibrium activity of magnesium is determined using the solubility product constant (Ksp) for magnesium hydroxide, Mg(OH)2. The pH value indicates that the concentration of hydroxide ions (OH-) is significant, which affects the dissociation of magnesium ions in the solution. The calculation requires understanding the dissociation constant of water and the relationship between pH, pOH, and ion activities.

PREREQUISITES
  • Understanding of pH and pOH concepts
  • Knowledge of solubility product constants (Ksp)
  • Familiarity with chemical equilibrium principles
  • Basic skills in calculating ion concentrations from pH values
NEXT STEPS
  • Calculate the dissociation constant of water (Kw) at the given temperature
  • Learn how to apply the solubility product for Mg(OH)2 to find magnesium ion concentration
  • Study the relationship between pH, pOH, and ion activities in aqueous solutions
  • Explore the implications of high pH on metal solubility in natural waters
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Chemistry students, environmental scientists, and water quality analysts interested in understanding the chemical behavior of minerals in natural spring waters.

skyblu280
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Mg 2+ (aq) +2 OH- (aq)= Mg (OH)2 (s)


If I measure pH of springs near Jenner to be pH=9.5, what can you tell about the equilibrium activity (concentration) of magnesium in that solution? You need to calculate the dissociation constant of water.

Not sure how to start this? Any help
 
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Why do you ignore homework template? In hope nobody will realize? I should delete your post and send you a warning about ignoring forum rules.

What is activity of H+ in the water?

What is activity of OH- in the water?

Now use solubility product for Mg(OH)2.
 
hi,

Sorry, I really thought I put this in the Hw section under the sciences...
 

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