Chapter 10, Problem 10.108CP

(a)

Interpretation Introduction

Interpretation:

The balanced equation for the given reaction should be determined.

Concept Introduction:

Balanced Chemical equation: On accordance with law of conservation of mass, for any chemical reaction, total masses of reactants and products must be equal.

Reaction between Acid and Base: When an acid reacts with the base $H^{+}$ from acid and ${\text{OH}}^{\text{-}}$ from base are neutralized that result in formation of salt and water.

(b)

Interpretation Introduction

Interpretation:

The $\text{pH}$ solution prepared by reaction between water and sodium oxide should be determined.

Concept Introduction:

$\text{pH}$: The concentration of hydrogen ion is measured using $\text{pH}$ scale. The $\text{pH}$ of a solution is a figure that expresses the acidity or the alkalinity of a given solution.

It is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

$\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$

If the value of $\text{pH}$ is less than $7$, then the solution is acidic whereas if the value of $\text{pH}$ is greater than $7$, then the solution is basic.

(c)

Interpretation Introduction

Interpretation:

The $mL$ of $HCl$ required to neutralize the $NaOH$ solution should be determined.

Concept Introduction:

Normality: It generally expresses the concentration of acid or base as equivalents of acid or base present in one liter of the solution.

$\text{Normality}\left(\text{N}\right)\text{=}\frac{\text{Equivalents of acid/base}}{\text{Liters of solution}}$

Equivalent of Acid: Generally, 1 equivalent of ion is the number of ions which has charge of one mole. In case of acids positive charge is of interest therefore, one equivalent of acid consists of 1 mole of $H^{+}$ ions.

Equivalent of Base: In case of bases negative charge is of interest therefore, one equivalent of base consists of 1 mole of $O{H}^{-}$ ions.

$\text{Bronsted-Lowry Acids}$: If a species loses a proton then it is considered as $\text{Bronsted-Lowry acid}\text{.}$

$\text{Bronsted-Lowry Base}$: If a species receives one proton, then it is considered as $\text{Bronsted-Lowry base}\text{.}$

If a base receives one proton, then the formed species is a conjugate acid whereas an acid lose one proton, then the formed species is a conjugated base.