Chapter 10.7, Problem 10.19P

(a)

Interpretation Introduction

Interpretation:

The normality for $5gofHN{O}_3$ diluted to $300mL$ of water 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.

(b)

Interpretation Introduction

Interpretation:

The normality for $12.5gofCa{\left(OH\right)}_2$ diluted to $300mL$ of water 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.

(c)

Interpretation Introduction

Interpretation:

The normality for $4.5gof{H}_{3}P{O}_4$ diluted to $300mL$ of water 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.