Chapter 15, Problem 15.50P

a)

Interpretation Introduction

Interpretation:

The activity of ${\text{Ca}}^{\text{2+}}$ in the calcium citrate solution has to be calculated.

Concept Introduction:

Calibrating a glass electrode:

When you calibrate an electrode with standard buffers, to calculate the voltage with each buffer. The pH of buffer $\text{S1}$ is ${\text{pH}}_{\text{S1}}$ and measured electrode potential in that buffer is ${\text{E}}_{\text{S1}}$.

The slope of the line is

$\text{slope=}\frac{{\text{E}}_{\text{2}}{\text{-E}}_{\text{1}}}{\text{log}{\text{Α}}_{\text{2}}{\text{-logA}}_{\text{1}}}$

b)

Interpretation Introduction

Interpretation:

The formation constant ${\text{K}}_{\text{f}}$, for ${\text{CaA}}^{\text{-}}$ has to be calculated.

Concept Introduction:

Formation constant:

The general form of a problem where the problem has the relation between concentrations of the reactants and products,

${\text{K}}_{\text{f}}\text{=}\frac{\left[{\text{CaA}}^{\text{-}}\right]{\text{γ}}_{{\text{CaA}}^{\text{-}}}}{\left[{\text{Ca}}^{\text{2+}}\right]{\text{γ}}_{{\text{Ca}}^{\text{2+}}}\left[{\text{A}}^{\text{3-}}\right]{\text{γ}}_{{\text{A}}^{\text{3-}}}}$

Where,

$\text{K}$= formation constant