Chapter 10, Problem 10.37UKC

Interpretation Introduction

Interpretation:

The concentration for base required to neutralize 1M acid should be determined considering both volumes are equal.

Concept Introduction:

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.

Titration: It is a quantitative analysis method used to express the concentration of acid or base present in the solution.

For an acid-base titration ${\left(Eq\right)}_{acid}={\left(Eq\right)}_{base}$

That is,

$\begin{array}{l}{N}_{acid}\times V_{acid}=N_{base}\times V_{base}\\ where,\\ N=Normality\\ V=Volume\end{array}$

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

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

Molarity: The concentration for solutions is expressed in terms of molarity as follows,

$\text{Molarity = }\frac{\text{No}\text{. of moles of solute}}{\text{Volume of solution in L}}$

The normality for any acid or base equals the molarity times of the number of ${\text{H}}^{\text{+}}\text{and}{\text{OH}}^{\text{-}}$ correspondingly.

Equivalent of Acid: Generally, 1 equivalent of ion is the number of ions which has charge of one mole.

$\text{Bronsted-Lowry Acids}$: 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 $\text{Bronsted-Lowry base}\text{.}$