To Do

1. Introduce r(B,A) in The Mole

This is necessary in the context of number of atoms to particle

Example: Water (H₂O) has 3 atoms per molecule (or 3 moles of atoms per mole of molecules).

\[ \begin{align*} N(\mathrm{atoms}) &= n(\mathrm{atoms}) ~ N_{\mathrm{A}} \\[1.5ex] &= n(\mathrm{H_2O}) ~ r(\mathrm{atoms,H_2O}) ~ N_{\mathrm{A}} \\[1.5ex] &= 1~\mathrm{mol~H_2O} \left ( \dfrac{3~\mathrm{mol~atoms}}{\mathrm{mol~H_2O}}\right ) \left ( \dfrac{6.02\bar{2} \times 10^{23}}{\mathrm{mol}} \right ) \\[1.5ex] &= 1.80\bar{6}60\times 10^{24}~\mathrm{atoms} \\[1.5ex] &= 1.807\times 10^{24}~\mathrm{atoms} \end{align*} \]

2. Create “Concentration” and “Dilution” sections in Concentration

amount concentration
amount-of-substance concentration
molar concentration
molarity (depricated)

3. Finish reviewing Practice 05 problems.

4. Properly format all Molarity units with smallcaps (HTML and LaTeX)

Include callout box that compares 0.150 M to 0.150 M (latter is ubiquitous; former is official)

\[ \begin{align*} &= 0.150~\class{mjx-molar}{\mathrm{M}} \end{align*} \]

A 0.150 M aqueous solution of HCl…

5. LaTeX fraction formatting – use \displaystyle

Use \displaystyle when a denominator has a superscript following a subscript

\[ \dfrac{\mathrm{mol~H_2O}}{\mathrm{NH_4{^+}}} \]

\[ \dfrac{\mathrm{mol~H_2O}}{\displaystyle \mathrm{NH_4{^+}}} \]

6. Square brackets not molarity universally

IUPAC technically reserves bracket notation [X] to mean the concentration of species X relative to the standard concentration (which is usually 1 mol/L), making it a dimensionless quantity for use in equilibrium constant expressions.