Potassium bromide formula

Potassium Bromide Potassium bromide is a colourless crystal and also typically odourless compounds. It is pungent bitter in taste with saline flavor. In the aqueous solution the pH level of potassium chromate is maintained at 7. It has consists of potassium cations and bromide anions. Moreover it could be lead to the quickly disassociated with the ionic salts and disappears within the minutes. If you consumed at more concentrations it will lead to the irritating the mucous membrances. The systematic IUPAC name is known as potassium bromide . The chemical or molecular formula of potassium bromide is KBr. Structural Formula This is the structural formula of the potassium bromide: Chemical Formula The chemical formula of the Potassium bromide is KBr. Preparation Method It is prepared by the traditional method by the reaction of potassium carbonate is reacted with the iron bromide and it undergoes to treating with the scrap iron with excess chemical of bromine. The carbon dioxide is given as the byproduct. It can be easily converting the potassium bromide to the potassium nitrate. In the aqeous solution the potassium bromide is reacted with the silver nitrate then it is the formation of potassium nitrate and silver bromide. Learn More: Sodium Bromide, Formula, Preparation Method, Chemical Properties 4 K 2CO 3 + Fe 3Br 8 → 8KBr + Fe 3O 4 + 4CO 2 Physical Properties Melting point 1346 C Boiling point 2615 C Molecular weight 119.002g/mol Density 2.257g/cm 3 Solubility in water 53...

Potassium Bromide - KBr What is Potassium Bromide? KBr is a salt which is widely used as a sedative and as an anticonvulsant with the chemical name Potassium Bromide. Potassium Bromide is also called Bromide salt of potassium or Kalii bromidum or Tripotassium tribromide. The potassium bromide salt is odourless and comes in the form of white crystalline powder, colourless crystals, or white granular solid with a pungent bitter saline taste. Aqueous solutions of KBr have a pH value of 7. Table of Contents • • • • • • • Properties of Potassium Bromide – KBr KBr Potassium Bromide Molecular weight of KBr 119.002 g/mol Density of Potassium Bromide 2.74 g/cm 3 Melting point of Potassium Bromide 734 °C Boiling point of Potassium Bromide 1,435 °C Potassium Bromide Structure – KBr Potassium Bromide Structure – KBr KBr Uses (Potassium Bromide) • Potassium Bromide is used to manufacture photographic papers and plates. • Used as a laboratory agent. • Used as a heat stabiliser for nylon. • Used as a Sedative. • Used as an anticonvulsant. • Used in the water treatment of aquariums • Used to manufacture chemicals. • Used as plasticizers. Production of Potassium Bromide One of the traditional methods of producing KBr is by reacting potassium carbonate with an iron (III, II) bromide, Fe3Br8, produced by treating scrap iron in water with excess bromine. The chemical equation for the same is given as follows: 4 K 2CO 3 + Fe 3Br 8 → 8 KBr + Fe 3O 4 + 4 CO 2 Potassium Bromide Reaction...

Formula Information Click on the component link for advanced information from the physicochemical database. Use the document link to view/download the complete formulation document in Adobe Acrobat (.pdf) format. Name: Potassium Bromide 250-mg/mL Oral Solution, Preserved, Veterinary FormulaNumber: 1978 Synonyms: KBr Solution; KBr 25% Solution Components: Document:

Atoms are electrically neutral because the number of protons, which carry a 1+ charge, in the nucleus of an atom is equal to the number of electrons, which carry a 1- charge, in the atom. The result is that the total positive charge of the protons cancels out the total negative charge of the electrons so that the net charge of the atom is zero. Most atoms, however, can either gain or lose electrons; when they do so, the number of electrons becomes different from the number of protons in the nucleus. The resulting charged species is called an ion. The opposite process can also occur. When a neutral atom gains one or more electrons, the number of electrons increases while the number of protons in the nucleus remains the same. The result is that the atom becomes an anion—an ion with a net negative charge. We can illustrate this by examining some very simple cations and anions, those formed when a single hydrogen atom loses or gains an electron. Note: Hydrogen is actually somewhat unusual in that it readily forms both cations and anions. Most elements much prefer to form only one or the other. In terms of its electron configuration, can you explain why hydrogen can form both cations and anions? Feel free to post in the comments at the end of the article! H + ~~~~~~~~~\text^-~~~~~~~~~~~~~~~~~~~ H − space, space, space, space, space, space, space, space, space, space, space, space, space, space, space, space, space, space, start text, H, end text, start superscript, minus, end s...

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• Experimental Physico-chemical Properties • Experimental Melting Point: 730 °C Alfa Aesar 730 °C OU Chemical Safety Data (No longer updated) 730 °C Alfa Aesar 734 °C Oakwood 734 °C FooDB 734 °C Parchem – fine & specialty chemicals 734 °C Sigma-Aldrich 730 °C Strem 734 °C Kaye & Laby (No longer updated) 734 °C Oakwood • Experimental Boiling Point: 1435 °C Alfa Aesar 1380 °C OU Chemical Safety Data (No longer updated) 1435 °C Alfa Aesar 1435 °C FooDB 58.8 °C Parchem – fine & specialty chemicals 1435 °C Strem 1435 °C / 760 mmHg Kaye & Laby (No longer updated) • Experimental Refraction Index: 1.559 Alfa Aesar 1.559 Parchem – fine & specialty chemicals • Experimental Solubility: 104% w/w in 100?C water Kaye & Laby (No longer updated) 65% w/w in 20?C water Kaye & Laby (No longer updated) Freely soluble in water. Soluble in alcohol, glycerol Alfa Aesar slightly soluble in ethanol Kaye & Laby (No longer updated) slightly soluble in ether Kaye & Laby (No longer updated) • Experimental Density: 2.75 g/mL Alfa Aesar 2.75 g/mL Oakwood 3.119 g/l Parchem – fine & specialty chemicals 2.75 g/mL / 25 °C Kaye & Laby (No longer updated) • Miscellaneous • Appearance: odourless white or colourless crystalline solid OU Chemical Safety Data (No longer updated) • Stability: Stable. Incompatible with strong oxidizing agents, strongacids, bromine trifluoride and bromine trichloride. OU Chemical Safety Data (No longer updated) • Toxicity: Inorganic Compound; Bromide Compound; Industrial/Workplace T...