Chemical equilibrium concentrations

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The discussion centers on determining equilibrium concentrations for the reaction involving magnesium hydroxide, given an equilibrium constant (K = 2.6 x 10^-6). It is clarified that magnesium hydroxide is a solid, and its activity is considered to be 1, negating the need for an ICE table. The correct balanced reaction should be Mg(OH)2 <===> Mg2+ + 2OH-, leading to a different equilibrium expression. Participants point out that the initial values provided for K are inconsistent with chemical reality, suggesting that the actual K should be much smaller, around 10^-10 or 10^-11. This discrepancy indicates that the calculated concentrations from the original problem are likely incorrect.
cj2222
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I have a problem in which It asks to find the equilibrium concentrations but it only give the value of the equilibrium constant and the chemical equation. Is this even possible to solve or does it not have enough information?

Here is the problem

Determine the equilibrium concentrations for the reaction below. K = 2.6 x 10-6.

Mg2+ + 2OH- <====> Mg(OH-) (solid)
 
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Mg(OH-) or Mg(OH)2?

Write expression for the equilibrium constant. Is there any dependence between concentrations of the ions produced when solid dissolves?
 
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Can you use 1 as the equilibrium concentration of Mg(OH)2 and use this on the ICE table to find the other equilibrium concentrations or would this give you the wrong answer?

because k = 1/[Mg2+][OH-]

or would the answer be

1/(x)(2x)^2 = 2.6 x 10^-6

where x = the equilibrium concentration of Mg2+
 
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1 is OK, but not as a concentration - magnesium hydroxide is a solid, so its activity is assumed to be 1. There is no need for ICE table - as long as there is solid present, its activity is 1. Just 1.

Your k is wrong - please write balanced reaction of magnesium dissolution first, then use it to construct reaction quotient.
 
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Mg2+ + 2OH- <===> Mg(OH)2k = 1/[Mg2+][OH-]2

The concentrations of OH- is going to be 2 times the concentration of Mg2+

so 2.6 x 10-6 = 1/(x)(2x)2so x = 45.81

the concentration of Mg2+ is 45.81

the concentration of OH- is 91.62

Is this correct or not because I can't think of any other way to do it?
 
You are on the right track, but numbers you get are absurd (BTW, you should list units in your answer).

IMHO that's because your initial reaction equation and value given for k are not consistent with chemical reality, which is probably not your fault.
 
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yeah, the reaction is supposed to be reversed, k is correct.

The reaction is supposed to be


Mg(OH)2 <===> Mg2+ + 2OH-


which would give much smaller and more reasonable concentrations.
 
My sources give pKsp for Mg(OH)2 as something between 10 and 11, which means k should be around 10-10 or 10-11. 10-6 looks way too large.
 

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