How many moles of \(\mathrm{Ca}(\mathrm{OH})_{2}\) would it take to completely neutralize \(0.4\) mole of phosphoric acid, \(\mathrm{H}_{3} \mathrm{PO}_{4} ?\)

Mole calculation is essential in the field of chemistry for quantifying substances. One mole corresponds to Avogadro's number, which is approximately 6.022 x 10^23, representing the number of particles (usually atoms or molecules) in that sample. In the given exercise, we utilize mole calculation to determine how many moles of calcium hydroxide (\( \text{Ca(OH)}_2 \) ) are needed to neutralize a specific amount of phosphoric acid (\( \text{H}_3\text{PO}_4 \) ).

It's important to understand that the coefficients in a balanced chemical equation provide the mole ratios between reactants and products. Here, for every one mole of phosphoric acid, two moles of calcium hydroxide are required. When we're given 0.4 moles of phosphoric acid, we set up a simple proportional equation to find that 0.8 moles of calcium hydroxide are needed for complete neutralization.

Balanced chemical equations are the bedrock of stoichiometric calculations. They ensure that the Law of Conservation of Mass is satisfied, meaning that the number of atoms for each element is the same on both sides of the equation. The balanced equation in the exercise shows the reaction between phosphoric acid and calcium hydroxide.

The coefficients in front of the chemical formulas are like the recipe for the reaction; they tell you how much of each substance you need or will produce. In our example, the equation states that two moles of calcium hydroxide react with one mole of phosphoric acid to produce calcium phosphate and water. Without balancing, we cannot accurately determine how much of each reactant is needed or how much product is created.

Acid-base neutralization is a type of chemical reaction where an acid and a base react to form a salt and usually water. This process is crucial in various scientific and industrial processes. In the context of this exercise, phosphoric acid (\( \text{H}_3\text{PO}_4 \) ) is the acid, and calcium hydroxide (\( \text{Ca(OH)}_2 \) ) is the base. Upon reacting, they produce calcium phosphate and water, a typical outcome of a neutralization reaction.

The goal is often to determine the correct amounts of an acid and a base to mix so that they completely neutralize each other. This exercise demonstrated the fundamental stoichiometric concept that more moles of calcium hydroxide are required than moles of phosphoric acid because the acid has three hydrogen ions available for reaction, as opposed to the two hydroxide ions provided by the base.