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Let's start by understanding acid-base titration. It is a laboratory method used to determine the concentration of an acid or base in a solution by adding a known amount of titrant (acid or base) until the reaction reaches its end-point, typically indicated by a color change in an indicator.
During the titration process, an acid and a base react to form water and a salt, a process known as neutralization.
By using data from the titration, we can calculate the concentration of one of the solutions using the equation: \ \text{{N}}_1 \text{{V}}_1 = \text{{N}}_2 \text{{V}}_2, where \ \( N_1 \) and \( V_1 \) are the normality and volume of the titrant, and \( N_2 \) and \( V_2 \) are the normality and volume of the analyte.

A neutralization reaction occurs when an acid reacts with a base to form water and a salt.
In the exercise, \( \text{{H}}_2 \text{{SO}}_4 \) (sulfuric acid) and \( \text{{NaOH}} \) (sodium hydroxide) are involved in a neutralization reaction.
This reaction can be written as: \( \text{{H}}_2 \text{{SO}}_4 + 2 \text{{NaOH}} \rightarrow 2 \text{{H}}_2 \text{{O}} + \text{{Na}}_2 \text{{SO}}_4 \).
Here, 1 mole of \( \text{{H}}_2 \text{{SO}}_4 \) reacts with 2 moles of \( \text{{NaOH}} \) to produce water and sodium sulfate.
Each reactant is used up completely to form neutral water and a salt, indicating a stoichiometric completion where all equivalent acid and base are consumed.

The pH of a solution measures its acidity or basicity.
It is calculated using the formula: \( \text{{pH}} = -\log [\text{{H}}^+] \), where \( [\text{{H}}^+] \) is the concentration of hydrogen ions.
In neutralization, if equal amounts of a strong acid and strong base mix, the \( \text{{H}}^+ \) and \( \text{{OH}}^- \) ions completely neutralize each other, leading to a pH of 7.
For the exercise provided, after calculating the milliequivalents of both \( \text{{NaOH}} \) and \( \text{{H}}_2 \text{{SO}}_4 \), the solution is neutral with a pH of 7 since they neutralize each other completely.

Normality (N) and molarity (M) are both measures of concentration.
Molarity is the number of moles of solute per liter of solution: \( M = \frac{{moles\text{{ of solute}}}}{{liters \text{{ of solution}}}} \).
Normality is the gram equivalent weight of solute per liter of solution and takes into account the reactivity of the solute: \( N = \frac{{equivalents \text{{ of solute}}}}{{liters \text{{ of solution}}}} \).
For acids and bases, normality accounts for the number of protons or hydroxide ions a substance can donate or accept.
In the given exercise, we converted the molarity of \( \text{{H}}_2 \text{{SO}}_4 \) to normality, recognizing that it is a diprotic acid and thus its normality is twice its molarity.