Chapter 18.1, Problem 4PP

Interpretation Introduction

Interpretation:

Balanced equation for the given products of acid- base reaction is to be written and conjugate acid-base pairs are to be identified.

Concept introduction:

The concept of conjugate acid-base pair is given by Bronsted-Lowry.

According to it,

Acid is a substance which donate hydrogen ion and Base is a substance which accept hydrogen ion.

When acid donates $H^{+}$, the species form is conjugate base and when base accepts $H^{+}$, the species form is conjugate acid.

Answer to Problem 4PP

The balanced equation is:

$H_{2}O+HS{O}_4{}^{-}\to H_3{O}^{+}+S{O}_4{}^{2-}$

Conjugate acid: $H_3{O}^{+}$

Conjugate base: $S{O}_4{}^{2-}$

Explanation of Solution

The products of acid-base equation are:

$H_3{O}^{+}$, $S{O}_4{}^{2-}$

$H_3{O}^{+}$ is formed by accepting $H^{+}$ from $H_{2}O$ and $S{O}_4{}^{2-}$ is formed by losing $H^{+}$ from $HS{O}_4{}^{-}$

Therefore, equation is:

$H_{2}O+HS{O}_4{}^{-}\to H_3{O}^{+}+S{O}_4{}^{2-}$

Conjugate acid: $H_3{O}^{+}$

Conjugate base: $S{O}_4{}^{2-}$

Conclusion

Thus,

The balanced equation is:

$H_{2}O+HS{O}_4{}^{-}\to H_3{O}^{+}+S{O}_4{}^{2-}$

Conjugate acid: $H_3{O}^{+}$

Conjugate base: $S{O}_4{}^{2-}$