Chapter 18.3, Problem 18.5AFP

(a)

Interpretation Introduction

Interpretation:

The acid - base reaction from the given conjugate acid-base pair of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{3}}{\text{ / HSO}}_{\text{3}}^{\text{-}}{\text{ and HCO}}_{\text{3}}^{\text{-}}{\text{ / CO}}_{\text{3}}^{\text{2-}}$ has to be written with $\text{Kc > 1}$.

Concept introduction:

Conjugate acid-Base pairs:

The acid donates the proton to form its conjugate base and the base accepts a proton to form its conjugate acid.

When an acid is dissolved in water, the acid $\text{(HA)}$ donates a proton to water to form a new acid (conjugate acid) and a new base (conjugate base).

The pair of an Acid –Base differs by a proton called conjugated Acid-Base pair.

In acid – base reaction, if the stronger acid produces the weaker acid which tells that the reaction favors the products, and the $\text{Kc}$ value is greater than one $\left(\text{Kc > 1}\right)$. If the weaker acid produces the stronger acid which tells that the reaction favors the reactants, and the $\text{Kc}$ value is less than one $\left(\text{Kc < 1}\right)$.

(b)

Interpretation Introduction

Interpretation:

The acid - base reaction from the given conjugate acid-base pair of ${\text{HF / F}}_{}^{\text{-}}{\text{ and HCN / CN}}_{}^{\text{-}}$ has to be written with $\text{Kc < 1}$.

Concept introduction:

Conjugate acid-Base pairs:

The acid donates the proton to form its conjugate base and the base accepts a proton to form its conjugate acid.

When an acid is dissolved in water, the acid $\text{(HA)}$ donates a proton to water to form a new acid (conjugate acid) and a new base (conjugate base).

The pair of an Acid –Base differs by a proton called conjugated Acid-Base pair.

In acid – base reaction, if the stronger acid produces the weaker acid which tells that the reaction favors the products, and the $\text{Kc}$ value is greater than one $\left(\text{Kc > 1}\right)$. If the weaker acid produces the stronger acid which tells that the reaction favors the reactants, and the $\text{Kc}$ value is less than one $\left(\text{Kc < 1}\right)$.