chemistry stuff
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anyone can explain the difference between H2O(l) and H2O(aq)? aren't they the same?
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aqueous H2O = water dissolved in water?
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same, unless it's H³0+ (aq).
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if they are the same, why do they have 2 different symbols?
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eh..
aquerous means in water..
(l) also means in water..
except u always put H2O as (l).. -
pedantically,
(l) could be more to indicate that water, as a participating reagent, is in its liquid state
(aq) has a double meaning, inferring that water is reacting both in its liquid state and "dissolved" as H+ and O2- ions -
huh???
i thought (l) is because it is like distilled water, no ions disassociate
then aqueous will have
-confused- -
er, if you are O level, just take H20 as (l) can liao.
for A level it gets a bit more complicated. -
For me, I will put the state symbol of H2O as l. The state symbol (aq) refers to a solution that is dissolved in water. It makes no sense to say that H2O dissolves in H2O.
For example: HCL (aq) refers to hydrochloric acid while HCL (g) refers to hydrogen chloride gas. Hydrochloric acid is a product when hydrogen chloride is pumped and dissolved in water.
Hydrochloric acid has acidic properties while hydrogen chloride gas doesn't.
Thus, my stand on H2O(l) result. -
H2O is (l) since its in the liquid form, just like eg. NaCl(l) in molten state. (aq) is for substances dissolved in water eg. NaCl(aq) sodium chloride solution.
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O2-??Originally posted by poon cho tang:pedantically,
(l) could be more to indicate that water, as a participating reagent, is in its liquid state
(aq) has a double meaning, inferring that water is reacting both in its liquid state and "dissolved" as H+ and O2- ions
I thought it is OH-.
2H2O <--> H3O+ + OH-
How do we get oxide ion?
O2- + H2O <--> 2OH- ???
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1+1=2
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for o levels, no such thing as H2O (aq). aq means the compund has dissociated in a solvent, which is illogical for h2o as h2o cannot dissociate in h2o.Originally posted by th3m0ment:anyone can explain the difference between H2O(l) and H2O(aq)? aren't they the same?
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How about A Level?Originally posted by unclebutcher:for o levels, no such thing as H2O (aq). aq means the compund has dissociated in a solvent, which is illogical for h2o as h2o cannot dissociate in h2o.
I don't mind to learn more
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I think the term should be auto-protonation of water/self-ionization of water/auto-dissociation of water.
2H2O(l) <--> H3O+(aq) + OH-(aq) Kw = 1 x 10^-14
Kw is water dissociation constant. You can find more about this in acid-base equilibria. 
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When they put H2O(l), it usually mean the water does not take part in the chemical reaction.
Bluff you la.
Water(l) is put in there to confuse pple. -
But But But...Originally posted by HyuugaNeji:When they put H2O(l), it usually mean the water does not take part in the chemical reaction.
Bluff you la.
Water(l) is put in there to confuse pple.
Say Alkali metal react with water.
K(s) + H2O(l) --> KOH(aq) + H2(g)
So water take part in the chemical reaction right? -
I say usually ma. Not always.Originally posted by Darkness_hacker99:But But But...
Say Alkali metal react with water.
K(s) + H2O(l) --> KOH(aq) + H2(g)
So water take part in the chemical reaction right? -
I knowOriginally posted by HyuugaNeji:I say usually ma. Not always. -
This question is puzzling.
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If you want, explain it using equilibria. For simplicity, I will use H+ instead of H3O+.Originally posted by Darkness_hacker99:But But But...
Say Alkali metal react with water.
K(s) + H2O(l) --> KOH(aq) + H2(g)
So water take part in the chemical reaction right?
H2O <--> H+ + OH- Reaction 1 (equilibrium reaction)
2K(s) + 2H+(aq) --> 2K+(aq) + H2(g). reaction 2 (forward reaction)
This reaction will always go forward.
Since H+ is being consumed in reaction 2, concentration of H+ will decrease. As such, by Le Chartelier's Principle, the system will try to produce more H+ in reaction 1 so that the system reaches the equilibrium, by shifting the equilibrium of reaction forward (to the right) favouring production of H+ and OH-.