Hydronium Treatment: H3O+ vs. H+ Equilibrium Constants

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In summary, the equilibrium constant for the reaction 2 H2O = H3O+ + OH- is different from that of Kw, H2O = H+ + OH-, which is used to describe acid-base systems. However, there is no need for modifications in the process when using [H3O+] instead of [H+], as they are treated in the same manner. The change in labels is due to the belief that free protons do not exist in solution, making the use of the hydronium label more accurate.
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Big-Daddy
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Is it true that the reaction 2 H2O = H3O+ + OH- has a different equilibrium constant to that of Kw, H2O = H+ + OH- ? How can that be?

If we want a decent treatment of an acid-base system using [H3O+] rather than the less accurate [H+], what modifications do we have to make to the process used for the simple [H+] case?
 
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No modifications necessary, they are treated exactly the same. It's simply a matter of changing the labels because free protons are not thought to exist in solution such that it is more realistic to denote the proton by using the hydronium label.
 

1. What is Hydronium Treatment?

Hydronium Treatment is a process that involves the use of hydronium ions (H3O+) to treat various conditions, such as acidity in water or acid reflux in the human body.

2. What is the difference between H3O+ and H+?

H3O+ and H+ are both forms of hydrogen ions, but H3O+ is a hydronium ion that has an additional water molecule attached to it. This makes H3O+ more stable and less reactive compared to H+.

3. How do H3O+ and H+ affect the equilibrium constant?

In a solution with both H3O+ and H+ ions, the equilibrium constant is affected by the concentration of H3O+ rather than H+. This is because H3O+ is the more prevalent and stable form of hydrogen ions in aqueous solutions.

4. How does the concentration of H3O+ impact the acidity of a solution?

The concentration of H3O+ is directly related to the acidity of a solution. The higher the concentration of H3O+, the more acidic the solution is. This is because H3O+ ions are responsible for the acidic properties of a solution.

5. Can the equilibrium constant for H3O+ and H+ change?

Yes, the equilibrium constant for H3O+ and H+ can change depending on factors such as temperature, pressure, and the presence of other ions. These changes can shift the balance between H3O+ and H+ ions and affect the equilibrium constant.

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