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

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The discussion revolves around determining whether the equilibria of NH4F, (NH4)2S, and MgO in water favor products or reactants. For NH4F, it is established that the reaction favors reactants with a Keq of 8.5 x 10^-7 due to the hydrolysis of its ions, NH4+ and F-. The analysis of (NH4)2S and MgO follows similar principles, focusing on the dissociation and hydrolysis of the ions produced. The participants emphasize the importance of including water in the equilibria calculations, as it acts as an acid or base in these reactions. Overall, the discussion highlights the complexity of acid-base equilibria and the necessity of understanding hydrolysis to solve these problems effectively.
  • #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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