Chapter 14, Problem 14.139MP

Interpretation Introduction

Interpretation:

The pH of the solution and the equilibrium concentration of all the species present $\left(C{H}_{3}COOH,C{H}_{3}CO{O}^{-},N{H}_3,N{H}_4^{+},H_3{O}^{+},O{H}^{-}\right)$ have to be determined.

Concept Introduction:

• According to ideal gas law,

$\text{PV=nRT}$

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

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

• Weak Acids: Acids that do not easily dissociate into ions completely which has difficulty in proton donation are considered as weak acids. Weak acid forms stronger conjugated base
• Weak Base: Bases that has little affinity towards protons. Weak base forms stronger conjugated acid.
• The $\text{pH}$ of a solution is a figure that expresses the acidity or the alkalinity of a given solution.
• The relationship between pH with weak acid weak base is given by, $pH=-\frac{1}{2}\left[\log K_a+\log K_w-\log K_b\right]$