The Phosphate Formula, is also called the OrthoPhosphate Formula or the Phosphate ion formula. There is one central phosphorus atom in this salt of phosphoric acid, surrounded by four oxygen atoms in a tetrahedral shape. Phosphate salts are formed when a positively charged ion attaches to a negatively charged oxygen atom and forms an ionic compound. It is also found in the form of ADP, ATP, AMP, RNA, and DNA.
Water cannot dissolve most phosphates at standard temperatures and pressures. In contrast, the other elements are either slightly soluble or completely insoluble in water, except for sodium, rubidium, ammonium phosphates, potassium, and caesium.
Aqueous phosphate occurs in four types:
- Strongly basic solutions are dominated by the phosphate ion.
- Weakly basic conditions often produce the hydrogen phosphate ion.
- In weakly acidic situations, the dihydrogen phosphate ion is most common.
- In strongly acidic situations, trihydrogen phosphate is the main form.
Phosphate Formula Structure
In a tetrahedral shape, four oxygen atoms surround the phosphorus atom. It is common to find organic phosphates in the form of esters in nucleotides (e.g. AMP, ADP, and ATP) as well as in RNA and DNA. The phosphoanhydride bonds in ATP or ADP can be hydrolysed to release free orthophosphate anions. Several metabolic processes are powered by these phosphorylation and dephosphorylation reactions. ATP and ADP are considered high-energy phosphates, as are phosphagens in muscle tissue. These reactions also occur for the other nucleoside diphosphates and triphosphates. In biological systems, phosphates play an important role as structural materials in bones and teeth.
Physical Properties of Phosphate
- Phosphate has a molecular weight of 94.97 g/mol.
- There are four hydrogen bond acceptors in this molecule.
- As a conjugate acid phosphate, it contains hydrogen.
- It is very slightly soluble in water.
Chemical Properties of Phosphate
- When Phosphate is reacted with water, Hydrogen Phosphate (HPO4) and Hydroxide (OH–) are obtained.
- When phosphate is reacted with silver, Silver (I) Phosphate is obtained.
- When Phosphate is reacted with Nitric acid (HNO3), Nitrate (NO3) and Hydrogen Phosphate (HPO4) are obtained.
Uses of Phosphate
- In kinds of toothpaste, it acts as a polishing agent.
- It is used in various pharmaceutical products.
- It is also used in fire extinguishers.
- In the industrial sector, it is used as a cleaner.
- It is used for the making of pyrotechnics and fire shells.
FAQs (Frequently Asked Questions)
1. Is it essential for students to learn the concepts related to the Phosphate Formula?
Yes, the Phosphate Formula is one of the very essential topics for students to retain as Phosphate is one of the very critical compounds of Chemistry. For students to understand various chemical bonds of the subject, they should be thorough with the Phosphate Formula. Students can take assistance of the Extramarks website for further information related to this topic.
2. Are the concepts related to the Phosphate Formula difficult?
No, the concepts related to the Phosphate Formula are not challenging for students. They must thoroughly practice these concepts to be able to score well in their examinations.
3. How can students clear their doubts related to the Phosphate Formula?
Extramarks is a website that provides students with access to various learning modules such as Live Doubt Solving Sessions, K12 Live Classes and much more so that they can easily resolve their doubts and score well in any examinations. Furthermore, the learning website also provides learners with learning tools such as Complete Syllabus Coverage, In-Depth Performance Reports, Self-Learning App and much more. These learning tools are designed to help students have successful academic careers. Students can learn about the Phosphate Formula and other chemical formulas with the assistance of the resources provided by Extramarks.