Sodium Phosphate Formula

Sodium phosphate is an inorganic compound with sodium (Na⁺) cation and phosphate (PO₄^3-) anions. It is also known as Phospho soda. The molecular formula of sodium phosphate is Na₃PO₄. These salts can be found in both anhydrous (water-free) and hydrated forms, with hydrates being more common. Sodium phosphate is used in various applications, including food processing, water treatment, and pharmaceuticals. In this article, we will look into what Sodium Phosphate is, its structure, properties, reactions, uses, etc.

What is Sodium Phosphate?

Sodium Phosphate is an inorganic salt composed of sodium and phosphate ions. The molecular symbol of sodium phosphate is Na₃PO₄. Sodium phosphate is also called Trisodium Phosphate, Sodium Orthophosphate and Tribasic Sodium Phosphate. These salts can be found in both anhydrous (water-free) and hydrated forms, with hydrates being more common. Sodium phosphate is used in various applications, including food processing, water treatment, and pharmaceuticals. In food processing, sodium phosphates are used as emulsifiers, thickening agents, leavening agents, and pH control agents. They are also used in water treatment to control pH and as a mild laxative. In pharmaceuticals, sodium phosphates are used as buffers and chelating agents and in preparing other pharmaceutical compounds.

Sodium Phosphate Formula

The molecular of chemical formula of Sodium Phosphate is Na₃PO₄

Sodium Phosphate Molecular Mass

Molar mass of Sodium Phosphate is 163.94 g/mol

Types of Sodium Phosphate

The most common sodium phosphate salts are:

Monosodium Phosphate (MSP)

Also known as sodium dihydrogen phosphate (NaH₂PO₄), it comes in anhydrous, monohydrate, and dihydrate forms:

• Anhydrous formula: NaH₂PO₄
• Monohydrate formula: NaH₂PO₄·H₂O
• Dihydrate formula: NaH₂PO₄·2H₂O

Disodium Phosphate (DSP)

Also known as sodium hydrogen phosphate (Na₂HPO₄), it comes in anhydrous, heptahydrate, octahydrate, and dodecahydrate forms:

• Anhydrous formula: Na₂HPO₄
• Heptahydrate formula: Na₂HPO₄·2H₂O
• Octahydrate formula: Na₂HPO₄·8H₂O
• Dodecahydrate formula: Na₂HPO₄·12H₂O

Trisodium Phosphate (TSP)

Comes in anhydrous and various hydrated forms such as hemihydrate, hexahydrate, octahydrate, and dodecahydrate:

• Anhydrous formula: Na₃PO₄
• Hemihydrate formula: Na₃PO₄·0.5H₂O
• Hexahydrate formula: Na₃PO₄·6H₂O
• Octahydrate formula: Na₃PO₄·8H₂O
• Dodecahydrate formula: Na₃PO₄·12H₂O

Pyrophosphates (DIPs)

Examples include disodium pyrophosphate (Na₂H₂P₂O₇) and tetrasodium pyrophosphate (Na₄P₂O₇)

Polyphosphates

Examples include sodium tripolyphosphate (Na₅P₃O₁₀) and higher molecular weight polymers like Graham's salt (sodium hexametaphosphate)

Structure of Sodium Phosphate (Na3PO4)

Sodium phosphate (Na₃PO₄) is an ionic compound composed of sodium cations (Na⁺) and phosphate anions (PO₄^3-). The phosphate anion is covalent, while sodium forms sodium cations by losing one electron. In the structure of sodium phosphate, three sodium cations are attracted to one phosphate anion, resulting in a zero net charge. The compound exhibits an electrovalent chemical structure and appears as white or off-white crystals, granules, or powder.

Properties of Sodium Phosphate (Na₃PO₄)

The properties of sodium phosphate is as follows:

Physical Property

The physical properties of sodium phosphate (Na₃PO₄) are as follows:

• Appearance: Sodium phosphate appears as an off-white powder
• Solubility: Sodium phosphate is soluble in water
• Density: The density of sodium phosphate is approximately 1.62 g/cm³
• Melting Point: The melting point of sodium phosphate is 1,583 °C
• Boiling Point: Sodium phosphate has a boiling point of 100 °C

Chemical Properties

The chemical properties of sodium phosphate (Na₃PO₄) are as follows:

• Acid-Base Nature: Sodium phosphate is a salt that can act as a buffer, helping maintain a solution's pH.
• Chelating Agent: It can act as a chelating agent, binding to metal ions to form a stable, water-soluble complex.
• Reactivity: Sodium phosphate can undergo various chemical reactions, such as reacting with acids to form phosphoric acid and corresponding salt and reacting with metal ions to form insoluble precipitates.
• Sodium phosphate is an ionic compound with an electrovalent chemical structure.

Chemical Reactions of Sodium Phosphate(Na₃PO₄)

The chemical properties of sodium phosphate (Na₃PO₄) are as follows:

Reaction with Hydrochloric Acid: Sodium phosphate reacts with hydrochloric acid to form phosphoric acid and sodium chloride. The chemical reaction is illustrated below:

Na₃PO₄ + 3HCl → H₃PO₄ + 3NaCl

Reaction with Calcium Chloride: Sodium phosphate reacts with calcium chloride to form calcium phosphate and sodium chloride. The chemical reaction is illustrated below:

2Na₃PO₄ + 3CaCl₂ → 6NaCl + Ca₃ (PO₄)₂

Uses of Sodium Phosphate

The uses of Sodium Phosphate (Na₃PO₄) include:

• Short-term, local treatment of inflammation with neomycin as bacterial prevention, such as after glaucoma surgery or cataract surgery
• As a mild laxative, stimulating the emptying of the gallbladder
• One of the most palatable saline laxatives
• Used in the form of an oral solution as an anti-hypercalcemia
• Control of the pH of water hardness precipitation and as a control agent in mildly acidic solutions
• In the preparation of pharmaceutical compounds as buffers and the formulation of many pharmaceutically beneficial compounds
• In detergents to soften water and as an effective anti-rust solution
• In the food industry, as an emulsifier, thickening agent, and starting agent for baked goods
• In the control of pH in processed foods

Environmental Impact of Sodium Phosphate (Na₃PO₄)

Here are the environmental impacts of Sodium Phosphate (Na3PO4) in pointer format:

• Sodium Phosphate can cause skin and eye irritation and burns, respiratory tract irritation, and other acute health effects. Chronic health effects such as cancer can occur at some time after exposure to sodium phosphate and can last for months or years.
• Sodium Phosphate can cause eutrophication of water bodies, acidification of soil, and accumulation of organisms during its use.
• Sodium Phosphate can cause the imbalance of phosphorus and sodium in the organism, causing hyperphosphatemia, hypernatremia, calcium and phosphorus deposition, renal function damage, hypertension, and other problems affecting the organism's health.
• Sodium Phosphate can cause soil acidification and adversely affect the activity and diversity of soil microorganisms if the amount of sodium phosphate applied is too large.