Does sodium hydroxide (NaOH) participate in H-bonding?
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argh.. people..
theres no point in hydrogen bonding if there's already ionic bonding present. in liquid/molten NaOH it will be a verrryy high melting point solid or very high boiling point liquid because of the ionic lattice. hydrogen bonding means nothing when you have these really strong bonds.
if you put it in water... I don't see why it wouldn't hydrogen bond.. but think of the concentration that you will need to make appreciable hydrogen bonding. whenever we talk about hydrogen bonding we talk in terms of solvents.. like H2O or ethanol or propionioc acid. There are bajillions of molecules, and yes they will hydrogen bond.. if you put NaOH.. to even get 1M, you will need a **** load of NaOH in solution... the pH will be like 13-14.. destructive...
theres no point in hydrogen bonding if there's already ionic bonding present. in liquid/molten NaOH it will be a verrryy high melting point solid or very high boiling point liquid because of the ionic lattice. hydrogen bonding means nothing when you have these really strong bonds.
if you put it in water... I don't see why it wouldn't hydrogen bond.. but think of the concentration that you will need to make appreciable hydrogen bonding. whenever we talk about hydrogen bonding we talk in terms of solvents.. like H2O or ethanol or propionioc acid. There are bajillions of molecules, and yes they will hydrogen bond.. if you put NaOH.. to even get 1M, you will need a **** load of NaOH in solution... the pH will be like 13-14.. destructive...
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According to http://en.wikipedia.org/wiki/Hydroxide
"In aqueous solution the hydroxide ion forms strong hydrogen bonds with water molecules. A consequence of this is that concentrated solutions of sodium hydroxide have high viscosity due to the formation of an extended network of hydrogen bonds as in hydrogen fluoride solutions."
"In aqueous solution the hydroxide ion forms strong hydrogen bonds with water molecules. A consequence of this is that concentrated solutions of sodium hydroxide have high viscosity due to the formation of an extended network of hydrogen bonds as in hydrogen fluoride solutions."
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Wouldn't it be ion-dipole interaction rather than hydrogen bonding if you dissove NaOH in water?
Na+ and OH- dissociate and OH- can have attraction with partially polar hydrogen atoms.
Na+ and OH- dissociate and OH- can have attraction with partially polar hydrogen atoms.
I think OH becomes dissolved first. Then OH can grab the H+ ions and form water. More water formed means more H-bond, thus increasing viscosity as L St Pierre said. So I think, OH itself can't, but indirectly by forming water yes.
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