Chapter 14, Problem 14.130CHP

Interpretation Introduction

Interpretation:

The $\text{pH}$ and concentration of all species namely $H_3{O}^{+},O{H}^{-},HN{O}_2,N{O}_2^{-}andN{O}_3^{-}$ present in given solution should be determined.

Concept Introduction:

Moles: One mole is equivalent to the mass of the substance consists of same number of units equal to the atoms present in $\text{12}\text{g}$ of ${}^{\text{12}}\text{C}$.

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

$\text{pH}$: 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.

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

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