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Old Feb 1st 2018, 11:06 AM   #1
bhhg
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what definition of acid and base theory fits in potassium chloride + water reaction?

We've been asked to identify the acid and base in KCl+H2O with appropriate acid-base definition and only the reactants are given.

We've learnt the following theory in class, Arrhenius, Brønsted–Lowry,Solvent System, Lux-Flood, Lewis.

I think the completed equation would be KCl+6H2O→K(H2 O)6]^+ +Cl^-

It would not be Arrhenius because no H+ and OH- are produced.
It would not be Brønsted–Lowry because no protons are involved.
It would not be Lux-Flood because no oxides are involved.
It would not be Lewis because no Electron pair are involved.


It would likely to be Solvent System but I don't know if it classifies a solvent or not. I am not sure my balanced equation is correct.
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Old Jun 7th 2018, 10:56 AM   #2
adianadiadi
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Originally Posted by bhhg View Post
We've been asked to identify the acid and base in KCl+H2O with appropriate acid-base definition and only the reactants are given.

We've learnt the following theory in class, Arrhenius, Brønsted–Lowry,Solvent System, Lux-Flood, Lewis.

I think the completed equation would be KCl+6H2O→K(H2 O)6]^+ +Cl^-

It would not be Arrhenius because no H+ and OH- are produced.
It would not be Brønsted–Lowry because no protons are involved.
It would not be Lux-Flood because no oxides are involved.
It would not be Lewis because no Electron pair are involved.


It would likely to be Solvent System but I don't know if it classifies a solvent or not. I am not sure my balanced equation is correct.
K+ can accept electron pairs. for example from water. So it is a Lewi acid.
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