Water Autoprotolysis
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gracetran3d
- Posts: 39
- Joined: Mon Jan 09, 2023 9:53 am
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Ali Nosseir
- Posts: 55
- Joined: Mon Jan 09, 2023 8:32 am
Re: Water Autoprotolysis
Water autoprotolysis is the ionization reaction of water denoted by:
H2O <-> H^+ + OH^-. Where Kw = 10^-14 at 25 degrees C.
The H+ and OH- concentrations are equal at 10^-7M because the pH of pure water is always 7.
H2O <-> H^+ + OH^-. Where Kw = 10^-14 at 25 degrees C.
The H+ and OH- concentrations are equal at 10^-7M because the pH of pure water is always 7.
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Alyssa Cheung 3I
- Posts: 50
- Joined: Mon Jan 09, 2023 10:11 am
Re: Water Autoprotolysis
I think the equation for water autoprotolysis is more accurately written as:
2H2O(l)-->H3O+(aq)+OH-(aq)
It's important to have the 2 in front of the water because this equation is showing the reaction between two water molecules. Remember that water is amphiprotic, meaning it can act as both acid and base due to its H+ and OH-, thus in a solution of water, there are still water molecules interacting with one another in the form of the aforementioned chemical equation.
Your Kc=[H3O+][OH-]=Kw (we exclude H2O from the equation because it's liquid)
At 25*C, Kw=1.0x10^-14 and [H3O+]=[OH-]
2H2O(l)-->H3O+(aq)+OH-(aq)
It's important to have the 2 in front of the water because this equation is showing the reaction between two water molecules. Remember that water is amphiprotic, meaning it can act as both acid and base due to its H+ and OH-, thus in a solution of water, there are still water molecules interacting with one another in the form of the aforementioned chemical equation.
Your Kc=[H3O+][OH-]=Kw (we exclude H2O from the equation because it's liquid)
At 25*C, Kw=1.0x10^-14 and [H3O+]=[OH-]
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