Chapter 16, Problem 35E

Interpretation Introduction

(a)

Interpretation:

The solubility product of saturated solution of silver iodide is to be stated.

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. 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,

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

Interpretation Introduction

(b)

Interpretation:

The solubility product of saturated solution of silver chromate is to be stated.

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. 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,

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

Interpretation Introduction

(c)

Interpretation:

The solubility product of saturated solution of silver phosphate is to be stated.

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. 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,

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