Chemical terminology of acids and bases:

• Acidity of a base: Defined as the number of ionizable or replaceable hydroxide ($OH^-$) ions present in one molecule of that base, or the number of moles of $H^+$ ions required to completely neutralize one mole of the base. For example, $NaOH$ has an acidity of $1$, $Ca(OH)_2$ has an acidity of $2$, and $Al(OH)_3$ has an acidity of $3$.
• Basicity of an acid: Defined as the number of replaceable hydrogen ($H^+$) ions in an acid molecule (e.g., $HCl$ has basicity $1$, $H_2SO_4$ has basicity $2$).

Calculation of molar solution mass:

• Molarity ($M$) is defined as moles of solute per liter of solution:
  $$\text{Molarity } (M) = \frac{\text{Mass (g)}}{\text{Molecular Weight (g/mol)} \times \text{Volume (L)}}$$
• Molecular weight of sulfuric acid ($H_2SO_4$):
  $$\text{MW} = (2 \times 1.008) + 32.066 + (4 \times 16.000) = 98.08\text{ g/mol} \approx 98\text{ g/mol}$$
• For $1\text{ L}$ of a $1\text{ M}$ solution, mass required $= 1\text{ mol} \times 98\text{ g/mol} = 98\text{ g}$.

Absolute error formula:

• Absolute error ($E_a$) is given by the magnitude of difference between the experimental observed value ($X_o$) and the true/standard value ($X_t$):
  $$E_a = |X_o - X_t|$$
• Substituting values:
  $$E_a = |45.5\% - 46.0\%| = 0.5\% = 0.5$$