Chapter 10.9, Problem 2QQ

Interpretation Introduction

Interpretation:

Among the given options, the pH of the solution with ${\text{[OH}}^{-}]=1.0\times {10}^{-6}$ has to be calculated.

Concept Introduction:

pOH definition:

The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion ${\text{[OH}}^{\text{-}}\text{]}$ concentration. pOH scale is analogous to pH scale.

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

Relationship between pH and pOH:

pOH is similar to pH.  The only difference is that in pOH the concentration of hydroxide ion is used as a scale while in pH, the concentration of hydronium ion is used.

The relationship between the hydronium ion concentration and the hydroxide ion concentration is given by the equation,

  $\text{pH}\text{+}\text{pOH}\text{=}\text{14,}\text{at}\text{25}{}^{\text{o}}\text{C}$

As pOH and pH are opposite scale, the total of both has to be equal to 14