Question

Label conjugate base, conjugate acid..?

Answer 1

Using the definitions...

Explanation:

`H_2S`- Bronsted-Lowry Acid, because it donates a proton (`H^+`)

`H_2O`- Bronsted-Lowry Base, because it accepts a proton (`H^+`)

`HS^-`- Bronsted-Lowry Conjugate Base, because it would have to accept a proton (`H^+`) to turn into `H_2S`

`H_3O^+`- Bronsted-Lowry Conjugate Acid, because it would have to donate a proton (`H^+`) to turn into `H_2O`

Answer 2

Here's what I get.

Explanation:

The equation for the reaction is

`underbrace("H"_2"S")_color(red)bb("BLA") + underbrace("H"_2"O")_color(red)bb("BLB") ⇌ underbrace("HS"^"-")_color(red)bb("CB") + underbrace("H"_3"O"^"+")_color(red)bb("CA")`

`"H"_2"S"color(white)(ml)` — BLA because it donates a proton to `"H"_2"O"`
`"H"_2"O"color(white)(m)` — BLB because it accepts a proton from `"H"_2"S"`

`"HS"^"-"color(white)(m)` — CB of `"H"_2"S"` because it has one less proton than `"H"_2"S"`
`"H"_3"O"^"+"` — CA of `"H"_2"O"` because it has one more proton than `"H"_2"O"`