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ionic equation

K2CrO4 (aq) + BaCl2 (aq) --> BaCrO4 + 2KCl

write the ionic equation of this please
Original post by whatcaniputhere
K2CrO4 (aq) + BaCl2 (aq) --> BaCrO4 + 2KCl

write the ionic equation of this please


These are all ionic chemicals. Therefore in solution, they will dissociate into ions:

K2CrO4 (aq) + BaCl2 (aq) ---> BaCrO4 (aq) + 2 KCl (aq)

becomes...

2 K+ (aq) + CrO42- (aq) + Ba2+ (aq) + 2 Cl- (aq) --> Ba2+ (aq) + CrO42- (aq) + 2 K+ (aq) + 2 Cl- (aq).

Do you know what to do after that?
Reply 2
Original post by whatcaniputhere
K2CrO4 (aq) + BaCl2 (aq) --> BaCrO4 + 2KCl

write the ionic equation of this please


Barium chromate is very insoluble in water(that is in aqueous solution, it is a solid).

what the other poster meant to post should be

2 K+ (aq) + CrO42- (aq) + Ba2+ (aq) + 2 Cl- (aq) --> BaCrO4 (s) + 2 K+ (aq) + 2 Cl- (aq).

you can work the rest out.
Reply 3
Original post by thegodofgod
These are all ionic chemicals. Therefore in solution, they will dissociate into ions:

K2CrO4 (aq) + BaCl2 (aq) ---> BaCrO4 (aq) + 2 KCl (aq)

becomes...

2 K+ (aq) + CrO42- (aq) + Ba2+ (aq) + 2 Cl- (aq) --> Ba2+ (aq) + CrO42- (aq) + 2 K+ (aq) + 2 Cl- (aq).

Do you know what to do after that?


just thought i should remind you in your equation, all are spectator ions, lol!:biggrin:
Original post by shengoc
just thought i should remind you in your equation, all are spectator ions, lol!:biggrin:


I know - there's no redox involved :s-smilie:
Reply 5
Original post by thegodofgod
I know - there's no redox involved :s-smilie:


yeah, but as you might know, barium sulphate is insoluble in water, chromate being of similar size to sulphate, one could guess barium chromate is also quite insoluble.

plus, i do know barium chromate is very insoluble in water.:biggrin:

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