[ch3mgirl]

If a solution of hypobroumous acid is added to a solution of sodium phosphate, a reaction takes place to a large extent to produce hydrogen phosphate ion and the hypobromite ion. Which base is weaker, the phosphate ion or the hypobromite ion?

My equation I came up with is:
HOBr(aq) + Na₃PO₄ (aq)  HPO₄^2- + OBr^-

I concluded that:
HOBr(aq) - stronger acid
Na₃PO₄ - stronger base
HPO₄^2- - conjugate acid (weaker acid)
OBr^- - conjugate base (weaker base)

Am I correct in thinking that OBr^- is the weaker base? My logic is that in a large extent reaction the reaction goes from stronger to weaker. Also, the stronger the acid, the weaker its conjugate base. Does this make sense?

[DevaDevil]

yes, you are correct in this

[ch3mgirl]

yes, you are correct in this

Thank you!