Chapter 2, Problem 8P

Summary Introduction

To determine: The $\text{pH}$ of the solution prepared by diluting $\text{3}\text{.0 mL}$ of $\text{2}\text{.5 M}$ $\text{HCl}$ to a final volume of $\text{100}\text{.0 mL}$ with ${\text{H}}_{\text{2}}\text{O}$.

Introduction:

The splitting of water results in the formation of two ionic species hydrogen ion and hydroxide ion. The hydrogen ions and hydroxide ions are released in equal number when the water is dissociated. The alkalinity or acidity of the solution is determined by the $\text{pH}$ (potential of hydrogen) of a solution.

The negative logarithm of the molar ion hydrogen (H⁺) ion concentration is called pH. It is calculated by the formula $\text{pH}=-{\text{log [H}}^{+}\text{]}$. The hydrogen ion concentration is calculated by the given $\text{pH}$ of the solution. The $\text{pH}$ of a solution is in the range of 0 to 14.