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VCE Stuff => VCE Science => VCE Mathematics/Science/Technology => VCE Subjects + Help => VCE Chemistry => Topic started by: methodsboy on January 04, 2009, 07:28:29 pm

Title: Ionic Equations
Post by: methodsboy on January 04, 2009, 07:28:29 pm: hey
i need urgent help ! :'(
i forgot how to write ionic equations for acid/base reactions.

Could someone please explain how to write an ionic equation for this acid/base reaction:

HNO3(aq) + NaOH(aq) --> NaNO3(aq) + H2O(l) :-\

Thankyou
Title: Re: Ionic Equations
Post by: osmoister on January 04, 2009, 07:42:14 pm: Quote from: methodsboy on January 04, 2009, 07:28:29 pm
hey
i need urgent help ! :'(
i forgot how to write ionic equations for acid/base reactions.

Could someone please explain how to write an ionic equation for this acid/base reaction:

HNO3(aq) + NaOH(aq) --> NaNO3(aq) + H2O(l) :-\

Thankyou

i'm not 100% certain ( just started studying it a week ago) but i think its:
H+ (aq) + oh-(aq) --> h2o(l)
Title: Re: Ionic Equations
Post by: NE2000 on January 04, 2009, 07:49:47 pm: Step one is to identify your aqueous solutions as ions and your molecules as molecules

So you have

$H^+ + NO_3^- + Na^+ + OH^- \rightarrow Na^+ + NO_3^- + H_2O(l)$

Then you eliminate the spectator ions, or those that remain unchanged either side of the equation. That leaves you with:

$H^+(aq) + OH^-(aq) \rightarrow H_2O(l)$
Title: Re: Ionic Equations
Post by: methodsboy on January 04, 2009, 09:01:15 pm: Quote from: NE2000 on January 04, 2009, 07:49:47 pm
Step one is to identify your aqueous solutions as ions and your molecules as molecules

So you have

$H^+ + NO_3^- + Na^+ + OH^- \rightarrow Na^+ + NO_3^- + H_2O(l)$

Then you eliminate the spectator ions, or those that remain unchanged either side of the equation. That leaves you with:

$H^+(aq) + OH^-(aq) \rightarrow H_2O(l)$
Thanks alot NE2000, pfft it was soo easy! lol i cnt believe i forgot how to do that.
Title: Re: Ionic Equations
Post by: AQ on January 09, 2009, 02:20:27 am: Quote from: NE2000 on January 04, 2009, 07:49:47 pm
Step one is to identify your aqueous solutions as ions and your molecules as molecules

So you have

$H^+ + NO_3^- + Na^+ + OH^- \rightarrow Na^+ + NO_3^- + H_2O(l)$

Then you eliminate the spectator ions, or those that remain unchanged either side of the equation. That leaves you with:

$H^+(aq) + OH^-(aq) \rightarrow H_2O(l)$

yeh thats right.
i loved this topic alot,.
Though i sort of forgot how to do it also.
when you said aqueous, then it came to my mind