Chapter 16, Problem 25E

Interpretation Introduction

(a)

Interpretation:

The equilibrium constant expression for the following reaction is to be stated.

${\text{HCHO}}_{\text{2}}\left(aq\right)\rightleftarrows {\text{H}}^{\text{+}}\left(aq\right)+{\text{CHO}}_2^{-}\left(aq\right)$

Concept introduction:

In a chemical reaction, when the rates of both forward and reverse reaction are equal, then the chemical reaction is said to be at equilibrium. They are reversible in nature. The equilibrium constant is denoted as $K_{eq}$. Mathematically, it is represented as the ratio of product concentration to reactant concentration raised to their stoichiometric coefficients, as shown below.

$K_{eq}=\frac{{\left[\text{Product}\text{concentration}\right]}^{\text{a}}}{{\left[\text{Reactant}\text{concentration}\right]}^{\text{b}}}$

Interpretation Introduction

(b)

Interpretation:

The equilibrium constant expression for the following reaction is to be stated.

${\text{H}}_{\text{2}}{\text{C}}_{\text{2}}{\text{O}}_{\text{4}}\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{HC}}_{\text{2}}{\text{O}}_4^{-}\left(aq\right)$

Concept introduction:

In a chemical reaction, when the rates of both forward and reverse reaction are equal, then the chemical reaction is said to be at equilibrium. They are reversible in nature. The equilibrium constant is denoted as $K_{eq}$. Mathematically, it is represented as the ratio of product concentration to reactant concentration raised to their stoichiometric coefficients, as shown below.

$K_{eq}=\frac{{\left[\text{Product}\text{concentration}\right]}^{\text{a}}}{{\left[\text{Reactant}\text{concentration}\right]}^{\text{b}}}$

Interpretation Introduction

(c)

Interpretation:

The equilibrium constant expression for the following reaction is to be stated.

${\text{H}}_{\text{3}}{\text{C}}_{\text{6}}{\text{H}}_{\text{5}}{\text{O}}_{\text{7}}\left(aq\right)\rightleftarrows {\text{H}}^{+}\left(aq\right)+{\text{H}}_{\text{2}}{\text{C}}_{\text{6}}{\text{H}}_{\text{5}}{\text{O}}_7^{-}\left(aq\right)$

Concept introduction:

In a chemical reaction, when the rates of both forward and reverse reaction are equal, then the chemical reaction is said to be at equilibrium. They are reversible in nature. The equilibrium constant is denoted as $K_{eq}$. Mathematically, it is represented as the ratio of product concentration to reactant concentration raised to their stoichiometric coefficients, as shown below.

$K_{eq}=\frac{{\left[\text{Product}\text{concentration}\right]}^{\text{a}}}{{\left[\text{Reactant}\text{concentration}\right]}^{\text{b}}}$