Chapter 17, Problem 17.142MP

Interpretation Introduction

Interpretation:

The concentration of ${\text{Cit}}^{3-}$, ${\text{H}}_2{\text{Cit}}^{-}$, ${\text{HCit}}^{2-}$ and ${\text{H}}_3\text{Cit}$ is to be calculated.

Concept introduction:

The Henderson-Hasselbalch equation is as follows:

$\text{pH}={\text{pK}}_{\text{a}}+\log \frac{\left[\text{base}\right]}{\left[\text{acid}\right]}$

The molarity is the concentration of the solution and is equal to the number of moles of the solute dissolved in liter of the solution.

The formula to calculate molarity is given as follows:

$\text{Molarity}\left(\text{mol/L}\right)=\frac{\text{number of moles}}{\text{volume}\left(\text{L}\right)}$

The conversion factor to convert $\text{L}$ to $\text{mL}$ is as follows:

$1\text{ L}=\text{1000 mL}$

Negative logarithm of molar concentration of hydronium ion is called $\text{pH}$. The expression for $\text{pH}$ is as follows:

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

$K_{\text{a}}$ is defined as the acid dissociation constant in conjugate acid-base pairs.