Chapter 14.3, Problem 14.2PSP

Interpretation Introduction

Interpretation:

The more basic solution from $2.0\times {10}^{-5}molHBr$ in $1.00\text{L}$ solution and $\text{5}\text{.0×}{\text{10}}^{-\text{9}}{\text{ OH}}^{-}$ concentration has to be determined.

Concept Introduction:

$\text{pH}$ is an logarithmic expression to express a solution is acidic, basic or neutral. The $\text{pH}$ scale has values 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.

$\text{pH + pOH= 14}$

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

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

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

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