Chapter 24, Problem 47IAE

Interpretation Introduction

(a)

Interpretation:

The pH of the solution should be determined.

Concept introduction:

A complex ion is formed when a metal ion reacts with a Lewis base in solution. This reaction is defined in terms of chemical equilibrium. A complexion comprises of a ligand and a metal ion as a result of an interaction of Lewis acid-base.

The Metal ion which is positively charged functions as a Lewis acid and Lewis base or the ligand has one or more lone pairs of electrons. For example, Cu²+, which is a highly charged and small metal ion having a significant tendency to function as Lewis acids, consequently exhibiting the highest affinity to form complex ions.

The development of a complexion is a stepwise procedure, and every step has its equilibrium constant. When two of the equations are added together, the equilibrium constants multiply. The Equilibrium Constant reflects the concentration in a reaction, which is the molarity, written as moles per liter (M = mol/L).

$K=\frac{{[C]}^c{[D]}^d}{{[A]}^a{[B]}^b}$

The products of a reaction are present in the numerator, and the denominator has the reactants. The alphabets in upper-case are the molar concentrations of the reactants and products, and the alphabets in lower-case are the stoichiometric coefficients which balance the equation.

This implies that the pH of any solution is the log of the hydrogen ion concentration of that solution. For the calculation of pH, the log of the hydrogen ion concentration is selected, and the sign is reversed to obtain the answer.

Interpretation Introduction

(b)

Interpretation:

The concentration of ${[Fe{(H_{2}O)}_{5}OH]}^{2+}(aq)$ should be determined when the given solution is also 0.100 M HClO₄ (where ClO₄-does not complex with Fe³⁺).

Concept introduction:

A complex ion is formed when a metal ion reacts with a Lewis base in solution. This reaction is defined in terms of chemical equilibrium. A complexion comprises of a ligand and a metal ion as a result of an interaction of Lewis acid-base. The Metal ion which is positively charged functions as a Lewis acid and Lewis base or the ligand has one or more lone pairs of electrons. For example, Cu²+, which is a highly charged and small metal ion having a significant tendency to function as Lewis acids, consequently exhibiting the highest affinity to form complex ions.

The development of a complexion is a stepwise procedure, and every step has its equilibrium constant. When two of the equations are added together, the equilibrium constants multiply. The Equilibrium Constant reflects the concentration in a reaction, which is the molarity, written as moles per liter (M = mol/L).

The products of a reaction are present in the numerator, and the denominator has the reactants. The alphabets in upper-case are the molar concentrations of the reactants and products, and the alphabets in lower-case are the stoichiometric coefficients which balance the equation.

$K=\frac{{[C]}^c{[D]}^d}{{[A]}^a{[B]}^b}$

$pH=-log\left[H+\right].$ This implies that the pH of any solution is the log of the hydrogen ion concentration of that solution. For the calculation of pH, the log of the hydrogen ion concentration is selected, and the sign is reversed to obtain the answer.

Interpretation Introduction

(c)

Interpretation:

Whether the pH of the solution can be maintained so that does not exceed 1×10-6 M.

Concept introduction:

A complex ion is formed when a metal ion reacts with a Lewis base in solution. This reaction is defined in terms of chemical equilibrium. A complexion comprises of a ligand and a metal ion as a result of an interaction of Lewis acid-base.

The Metal ion which is positively charged functions as a Lewis acid and Lewis base or the ligand has one or more lone pairs of electrons. For example, Cu²+, which is a highly charged and small metal ion having a significant tendency to function as Lewis acids, consequently exhibiting the highest affinity to form complex ions.

The development of a complexion is a stepwise procedure, and every step has its equilibrium constant. When two of the equations are added together, the equilibrium constants multiply. The Equilibrium Constant reflects the concentration in a reaction, which is the molarity, written as moles per liter (M = mol/L).

$K=\frac{{[C]}^c{[D]}^d}{{[A]}^a{[B]}^b}$

The products of a reaction are present in the numerator, and the denominator has the reactants. The alphabets in upper-case are the molar concentrations of the reactants and products, and the alphabets in lower-case are the stoichiometric coefficients which balance the equation.

$pH=-log\left[H+\right]$ This implies that the pH of any solution is the log of the hydrogen ion concentration of that solution. For the calculation of pH, the log of the hydrogen ion concentration is selected, and the sign is reversed to obtain the answer.