Chemical equilibrium system and where my ions went

[allywallyrus]

sorry if this has been asked before, i did a search and couldn't find any results.
Explain fully what happens when [tex]H^+[/tex] is added to a mixture containing [tex]BaCrO_4(s)[/tex] and [tex]CrO_4^2^-[/tex].

The overall equation of ions in this experiment is [tex]H^+(aq)~+~2CrO_4^2^-\rightleftharpoons~Cr_2O_7^2^-(aq)~+~OH^-(aq)[/tex]

when HCl is added to a solution of K2CrO4 and NaOH and Ba(NO3)2, the precipitate dissolves and the solution becomes orange. I am pretty stumped, but I am assuming K2CrO7 is present because it is orange in colour and that the precipitate from before becomes aqueous again but I am not sure what the percipitate is (possibly Ba(OH)2??) or what is involved in the reaction. any push in the right direction is very appreciated!

 

[chemisttree]

Ksp of barium hydroxide is 5 X 10^-3 and the Ksp of barium chromate is 2.2 X 10^-10.

Hope it helps.

 

[allywallyrus]

Ksp of barium hydroxide is 5 X 10^-3 and the Ksp of barium chromate is 2.2 X 10^-10.

Hope it helps.

i just realized i even identified barium chromate as a solid in my first post, hahaha :P
thank you anyway

so now my equation is looking more like HCl(aq) + BaCrO4 -> Cr2O7 + BaCl(aq) + H+

 

[Borek]

[tex]H^+(aq)~+~2CrO_4^2^-\rightleftharpoons~Cr_2O_7^2^-(aq)~+~OH^-(aq)[/tex]

It won't work this way. Think what will happen to produced OH^- in the presence of H⁺.

 

[allywallyrus]

It won't work this way. Think what will happen to produced OH^- in the presence of H⁺.

so we'd have H2O in the products instead, which makes more sense because this also balances nicely as well
i think this clears up where H+ ions were going, thanks :)

i don't suppose it would be a problem if i recycled this thread for questions on the same subject? i will probably have some more

 

[Borek]

No, you better start a new thread. Give it more informative subject.

 

[allywallyrus]

alright, thanks again