# How would you write the formula of the conjugate base of the Bronstead-Lowry acids H2SO3 and HI?

Jul 17, 2018

for ${H}_{2} S {O}_{3}$: the conjugate base is $H S {O}_{3}^{-}$

for $H I$: the conjugate base is ${I}^{-}$

#### Explanation:

Given: Bronstead-Lowry acids ${H}_{2} S {O}_{3}$ and $H I$

$B + H A \iff H {B}^{+} + {A}^{-}$

where $B$: base proton receiver; $\text{ } H A$ is the acid proton donor;

$H {B}^{+}$ is the conjugate acid; $\text{ } {A}^{-}$ is the conjugate base

For sulfurous acid $\left({H}_{2} S {O}_{3}\right)$:

${H}_{2} S {O}_{3} \left(a q\right) + {H}_{2} O \left(l\right) \iff {H}_{3} {O}^{+} \left(a q\right) + H S {O}_{3}^{-} \left(a q\right)$

the conjugate base is $H S {O}_{3}^{-}$

For hydroiodic acid $\left(H I\right)$:

$H I \left(a q\right) + {H}_{2} O \left(l\right) \iff {H}_{3} {O}^{+} \left(a q\right) + {I}^{-} \left(a q\right)$

the conjugate base is ${I}^{-}$