What volume of 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid? \(\mathrm{NaCl}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(l) \rightarrow \mathrm{HCl}(g)+\mathrm{NaHSO}_{4}(s)\)

Stoichiometry is the mathematical relationship between the quantities of reactants and products in a chemical reaction. It is based on the conservation of mass and the stoichiometric coefficients found in a balanced chemical equation. Each coefficient represents the number of moles of a given substance that participates in the reaction.

For instance, in the reaction between sodium chloride (NaCl) and sulfuric acid (H₂SO₄) to produce hydrochloric acid (HCl) and sodium hydrogen sulfate (NaHSO₄), the stoichiometric coefficients indicate a 1:1 mole ratio between NaCl and HCl. This means that for every mole of NaCl that reacts, one mole of HCl is produced. Understanding this concept allows us to predict the amount of HCl formed from a given amount of NaCl. When performing stoichiometry calculations, it’s important to start with a balanced chemical equation and use mole ratios to relate quantities of reactants to products.

A chemical reaction is a process that leads to the chemical transformation of one set of chemical substances to another. The substances that undergo the transformation are called reactants, and the substances formed as a result are called products. Chemical reactions are often described by chemical equations that show the reactants on the left side and the products on the right, with an arrow pointing from reactants to products.

In our example, NaCl reacts with H₂SO₄ and yields HCl and NaHSO₄. It's crucial to understand that the chemical equation must be balanced, which means the number of atoms for each element in the reactants must equal the number of atoms in the products. This is a reflection of the Law of Conservation of Mass, which states that matter cannot be created or destroyed in a chemical reaction. This balanced equation is the cornerstone for stoichiometry calculations, as it allows us to determine the mole ratio needed to calculate the volume of a particular solution.

Molar mass is the mass of one mole of a substance, usually measured in grams per mole (g/mol). It can be thought of as the bridge between the macroscopic world (grams, liters) and the microscopic world (molecules, atoms, moles). The molar mass allows us to convert between the mass of a substance and the number of moles, a fundamental step in stoichiometry calculations.

To find the molar mass of a compound, like sodium chloride (NaCl), sum up the atomic masses of all the atoms present in the molecule (found on the periodic table). For NaCl, we add the atomic mass of sodium (Na) to that of chlorine (Cl), resulting in approximately 58.44 g/mol. Knowing this value is crucial for solving stoichiometry problems, as it is used to convert the mass of NaCl into moles, which then allows for the determination of moles of other substances in the reaction, such as HCl. Accurately calculating molar masses is a fundamental skill for performing molarity calculations and other related stoichiometric analyses.