[hii_meliisssa]

This series of reactions proceeds predominately to the right as written.

a. HC₂H₃O₂ + NH₃   NH₄⁺ + C₂H₃O₂^-

b. HBr + H₂O   H₃O⁺ + Br^-

c. NH₄⁺ + Oh^-   NH₃ + H₂O

d. H₃O⁺ + C₂H₃O₂^-  
H₂O + HC₂H₃O₂

Arrange the bases NH₃, H₂O, OH^-,C₂H₃O₂^-, and Br^- in increasing order of basic strength. That is, place the weakest base first, the strongest base last. Beside the Bronsted bases, list the formulas of their conjugate acids.

Show as much work as possible.

[savy2020]

you seem to be new to the forum. please read Forum Rules
Atleast show your attempt at the solution . We'll be glad to help you

[hii_meliisssa]

better?


I'm not really sure how to show my attempt to the problem because I'm not exactly sure how to begin attempting it. :/ I would happily try if you lead me in the right direction.

[savy2020]

Well let me take an equation,
 HC2H3O2 + NH3   NH4+ + C2H3O2-
It is given that reaction is predominantly to right.
what does this tell? It means that NH3 accepts protons much readily than C2H3O2- and hence NH3 is a stronger base than C2H3O2-. Proceed in a similar way for all the 4 equations

[hii_meliisssa]

c. NH4+ + Oh-   NH3 + H2O

So, based on what you said about the first equation,
in this equation it would mean H20 is a stronger base than NH3?

and then I would continue from there?

[savy2020]

c. NH4+ + Oh-   NH3 + H2O

So, based on what you said about the first equation,
in this equation it would mean H20 is a stronger base than NH3?

Nope, Is H2O acting as a base here or an acid? Is it gaining H+{converted to H3O+} or losing{converted to OH-}?