Chapter 16, Problem 16.128SP

Interpretation Introduction

Interpretation:

Using the van’t Hoff equation and normal water $pH$ range has to be calculated    

Concept Information:

Van’t Hoff equation: This equation relates the temperature dependence of $Kp$ to the reaction enthalpy change.

$\ln \frac{K_2}{K_1}=-\frac{\Delta H}{R}\left(\frac{1}{T_2}-\frac{1}{T_1}\right)$

OR

$\frac{d\ln Kp}{dt}=\frac{{\Delta }_{f}H°}{R{T}^2}$

pH definition:

The concentration of hydrogen ion is measured using $\text{pH}$ scale.  The acidity of aqueous solution is expressed by $\text{pH}$ scale.

The $\text{pH}$ of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

  $\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$