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Phosphoric acid, with the chemical formula \( \mathrm{H}_3 \mathrm{PO}_4 \), is a common inorganic acid used in various chemical applications. It is a triprotic acid, meaning it has three hydrogen atoms that can potentially dissociate as hydrogen ions \( \text{H}^+ \). This property makes it highly versatile, as it can participate in different reactions depending on the chemical circumstances. In its pure form, phosphoric acid is a crystalline solid at room temperature, but it is usually encountered in liquid form as aqueous solutions. Understanding the behavior of phosphoric acid in chemical reactions is crucial for various industrial processes, such as fertilizer production and metal treatment.

Chemical reactions involve the transformation of one or more substances into new substances through the breaking and forming of chemical bonds. In the reaction given, phosphoric acid \( \mathrm{H}_3 \mathrm{PO}_4 \) and sodium hydroxide \( \mathrm{NaOH} \) are the reactants. The product formed by this specific reaction includes sodium dihydrogen phosphate \( \mathrm{NaH}_2 \mathrm{PO}_4 \) and water \( \mathrm{H}_2 \mathrm{O} \). This is an example of an acid-base reaction where an acid reacts with a base to produce salt and water. Such reactions are central to understanding chemical processes in biological systems and industrial settings.

Molecular weight, also known as molecular mass, is the sum of the atomic weights of all atoms in a molecule. It's expressed in units of grams per mole (g/mol), helping quantify substances in chemical reactions. To calculate the molecular weight of phosphoric acid \( \mathrm{H}_3 \mathrm{PO}_4 \), add up the atomic weights:

• 3 atoms of Hydrogen (H): \(3 \times 1 = 3\) g/mol
• 1 atom of Phosphorus (P): \(1 \times 31 = 31\) g/mol
• 4 atoms of Oxygen (O): \(4 \times 16 = 64\) g/mol

Combine these values for a total molecular weight of \(98\) g/mol. This value is vital for determining the equivalent weight and plays a crucial role in stoichiometry calculations within chemical reactions.

Acid-base reactions are a fundamental type of chemical reaction characterized by the transfer of \( \text{H}^+ \) ions from an acid to a base. In the reaction between phosphoric acid \( \mathrm{H}_3 \mathrm{PO}_4 \) and sodium hydroxide \( \mathrm{NaOH} \), the \( \text{H}^+ \) ion from phosphoric acid reacts with the \( \text{OH}^- \) ion from sodium hydroxide to form water. The remaining parts of the molecules combine to form sodium dihydrogen phosphate. This exchange of ions emphasizes the versatile nature of acids in donating protons and bases in accepting them, which is a key concept in the study of chemistry. Understanding acid-base reactions is essential for grasping broader chemical phenomena, such as buffer solutions and the pH scale.