Chapter 15, Problem 15.69SP

Interpretation Introduction

Interpretation:

We are given the equilibrium constant for water at elevated temperature and pressure. From this value, we must use the relationship between K_wand hydroxide and hydronium to find the concentrations of each species which can determine if the solution is acid, basic, or neutral.

Concept introduction:

• The equilibrium constant of an acid is referred to as the K_aand uses the formula: K_a= $\left[H^{+}\right]\left[A^{-}\right]/\left[HA\right]$
• The equilibrium constant of a base is referred to as the K_band uses the formula: K_b= $\left[B{H}^{+}\right]\left[O{H}^{-}\right]/\left[B\right]$
• We can use the equilibrium expression to determine the concentration of H+ ions which we use to calculate the pH of a solution using: $pH=-log\left[H^{+}\right]$
• We can determine the pOH and concentration of hydroxide from hydronium concentration using: $pH+pOH=14$
• The product of the base and acid dissociation constants provides the following formula: K_a? $K_b=1\times {10}^{-14}=K_w$

To classify:

The concentration of H₃O+ and OH- whether the solution is acidic, basic, or neutral.