Equilibrium of NH4F, (NH4)2S, and MgO in Water: Reactants or Products?

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SUMMARY

The discussion centers on the equilibria of NH4F, (NH4)2S, and MgO in water, specifically whether the resulting equilibria favor products or reactants. The key conclusion is that NH4F favors reactants with a Keq of 8.5 x 10-7, while MgO favors products with a Keq greater than 1022. The participants emphasize the importance of hydrolysis reactions and the role of spectator ions in determining the direction of equilibria. The correct hydrolysis equations for NH4+ and F- are crucial for accurate calculations.

PREREQUISITES
  • Understanding of chemical equilibria and the equilibrium constant (Keq)
  • Familiarity with hydrolysis reactions and the concept of spectator ions
  • Knowledge of weak acids and bases, including their dissociation in water
  • Ability to perform calculations involving Ka and Kb values
NEXT STEPS
  • Learn about the hydrolysis of ionic compounds in aqueous solutions
  • Study the calculation of equilibrium constants (Keq) for acid-base reactions
  • Explore the concepts of strong vs. weak acids and bases, particularly in the context of solubility equilibria
  • Investigate the role of water in acid-base equilibria and its impact on reaction direction
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Chemistry students, educators, and professionals involved in chemical equilibria, particularly those focusing on acid-base reactions and hydrolysis in aqueous solutions.

  • #31
Why would they give me such a question that doesn't fit with the method they want me to use ? and that question seems fishy to me because there is no product acid only the reactant acid (water) unless they assumed something that makes the answer turn out to be inequality. And that assumption they think I should know which I really really really really don't know. I've tried and tried until my personality split and still cannot figure out how they came up with answer like that.

if there is anyone else on this forum that knows why the answer is an inequality then please help me with it. Your help is greatly appreciated but I am still not going to leave this question alone. And one thing I still can't figure out is how did they come up with answer as large as to the magnitude of 22 !

Nothing makes sense to me with that question.
 
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  • #32
As mentioned before, this question is more than just acid-base equlibria. Take into account that Mg(OH)2 has a low Ksp as well, so consider its solubility equilibria.

I'm not sure how they got that number, but you can imagine that it'll be huge. Any OH- produced will precipitate out, lowering OH- concentration and driving the reaction forward to a virtual completion.
 
  • #33
Do I just leave that question then?
 
  • #34
Has anyone come across a question like this?
 

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