Chapter 14, Problem 14.127CHP

Interpretation Introduction

Interpretation:

The $\text{pH}$ and concentration of all the species present in $0.25\text{M}$ ${\text{H}}_{\text{2}}{\text{SO}}_{\text{3}}\text{and}{{\text{(NH}}_{\text{4}}\text{)}}_{\text{2}}{\text{SO}}_{\text{3}}$ has to be calculated.

Concept Introduction:

$\text{pH}$ is an logarithmic expression to express a solution is acidic, basic or neutral.  $\text{pH}$ scale values lies between 1-14 and on which 7 is neutral, below 7 values are more acidic in nature and above 7 values are more basic in nature.

$\text{pH + pOH= 14}$

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

$\left[{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\right]{\text{= antilog(-pH) =10}}^{\text{-pH}}$

$\text{pOH = -log}\left[{\text{OH}}^{-}\right]$

$\left[{\text{OH}}^{-}\right]{\text{= antilog(-pOH) =10}}^{\text{-pOH}}$

Percent dissociation:

It is defined as concentration of dissociated acid divided by the concentration of the acid times $100\%$.

$\text{Percent}\text{dissociation =}\frac{{\left[\text{HF}\right]}_{\text{dissociated}}}{{\left[\text{HA}\right]}_{\text{initial}}}\times 100\%$