[whatcaniputhere]

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

write the ionic equation of this please

[thegodofgod]

(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:

K₂CrO_{4 (aq)} + BaCl_{2 (aq)} ---> BaCrO_{4 (aq)} + 2 KCl _(aq)

becomes...

2 K⁺ _(aq) + CrO₄^2- _(aq) + Ba²⁺ _(aq) + 2 Cl^- _(aq) --> Ba²⁺ _(aq) + CrO₄^2- _(aq) + 2 K⁺ _(aq) + 2 Cl^- _(aq).

Do you know what to do after that?

[shengoc]

(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.

[shengoc]

(Original post by thegodofgod)
These are all ionic chemicals. Therefore in solution, they will dissociate into ions:

K₂CrO_{4 (aq)} + BaCl_{2 (aq)} ---> BaCrO_{4 (aq)} + 2 KCl _(aq)

becomes...

2 K⁺ _(aq) + CrO₄^2- _(aq) + Ba²⁺ _(aq) + 2 Cl^- _(aq) --> Ba²⁺ _(aq) + CrO₄^2- _(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!

[thegodofgod]

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

I know - there's no redox involved

[shengoc]

(Original post by thegodofgod)
I know - there's no redox involved

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.