Ammonium Iodide Extra Pure – 250gm Packs

Ammonium Iodide is an inorganic ionic compound composed of ammonium and iodide ions, with the chemical formula NH₄I and a molecular weight of 144.94 g/mol. It is a white crystalline solid that is highly soluble in water and can gradually develop a yellowish colour when exposed to air or light because of its sensitivity to oxidation and decomposition. Ammonium Iodide is used in appropriate laboratory investigations involving iodide chemistry, inorganic salt reactions, and the preparation of solutions containing iodide ions. It is relevant to college and university chemistry practicals, analytical studies, and research involving iodine-containing compounds and chemical reaction mechanisms. This 250 g pack is intended for laboratory applications where the compound’s identity and reagent specifications meet the requirements of the procedure. Appropriate protection from light, moisture, and air helps maintain its condition during storage.

Product Specifications

Key Features of Ammonium Iodide

• Defined ionic composition: Contains ammonium cations and iodide anions, making it relevant to experiments involving inorganic iodide salts.
• High water solubility: Dissolves readily in water for preparing solutions used in suitable laboratory investigations.
• Characteristic crystalline form: Occurs as a white crystalline solid and may develop a yellowish tint during storage because of its sensitivity to air and light.
• Reactivity of iodide ions: Supports appropriate chemical investigations involving iodide reactions, redox processes, and the formation of iodine-containing species.
• Versatile laboratory reagent: Can be used in educational and research procedures when its grade and specifications meet the analytical or experimental requirements.

Laboratory Applications of Ammonium Iodide

• Inorganic chemistry practicals: Used in supervised college and university experiments to study the properties and reactions of ammonium and iodide ions.
• Qualitative chemical analysis: Provides iodide ions for suitable identification reactions and investigations involving selected metal ions.
• Redox reaction studies: Supports appropriate experiments examining iodide oxidation and the formation of iodine under controlled reaction conditions.
• Analytical solution preparation: Used to prepare aqueous iodide-containing reagents for procedures that specify ammonium iodide as a reagent.
• Chemical research: May serve as an iodide source in selected reaction studies and investigations involving iodine-containing compounds, subject to the method and safety requirements.

Why Choose Lab Wale to Buy Ammonium Iodide

Lab Wale provides a convenient sourcing option for laboratory chemicals and scientific supplies used by schools, colleges, universities, research centres, and laboratory professionals. When purchasing Ammonium Iodide, checking the chemical name, CAS number, stated assay, grade, and intended application helps ensure that the reagent is appropriate for the planned procedure. Clear product identification and access to relevant technical and safety information support informed purchasing decisions. Laboratories should also consider the compound’s sensitivity to air and light when selecting suitable storage and handling practices.

Frequently Asked Questions About Ammonium Iodide

What is Ammonium Iodide used for in laboratories?

Ammonium Iodide is used in inorganic chemistry experiments, iodide-ion identification reactions, redox studies, and the preparation of suitable aqueous reagents. It can also serve as an iodide source in selected research procedures involving iodine-containing compounds, provided its specifications meet the requirements of the method.

What are the chemical formula and molecular weight of Ammonium Iodide?

The molecular formula is NH₄I, and its empirical formula is H₄IN. Its molecular weight is approximately 144.94 g/mol. The compound consists of ammonium ions and iodide ions in a 1:1 ratio, giving it an overall electrically neutral composition.

What is the CAS number of Ammonium Iodide?

The CAS Registry Number for Ammonium Iodide is 12027-06-4. This identifier helps distinguish the compound from other ammonium salts and iodine-containing reagents. It should be checked alongside the chemical name and molecular formula when ordering laboratory chemicals or preparing experimental documentation.

Why can Ammonium Iodide turn yellow during storage?

Ammonium Iodide can gradually develop a yellowish colour because it is sensitive to air and light, which can promote chemical changes and the formation of iodine-containing species. Keeping the container tightly closed and protected from light helps limit deterioration. Follow the product-specific storage recommendations for best handling practice.

How should Ammonium Iodide be stored and handled safely?

Store Ammonium Iodide in a tightly closed, compatible container in a cool, dry place protected from light and excessive exposure to air. Wear suitable gloves, protective clothing, and safety goggles, and avoid inhaling dust or contacting the eyes and skin. Consult the current Safety Data Sheet for detailed precautions.

Storage Conditions for Ammonium Iodide

Store Ammonium Iodide in a tightly sealed, compatible container in a cool, dry, well-ventilated area, protected from direct light and unnecessary exposure to air. A storage temperature below 25 °C is appropriate for many reagent specifications. Minimise moisture exposure and keep the material away from incompatible chemicals. Close the container promptly after use to help limit oxidation and yellowing.

Precautions for Handling Ammonium Iodide

Review the current Safety Data Sheet before use and wear suitable chemical-resistant gloves, protective clothing, and safety goggles. Avoid generating or inhaling dust and prevent contact with the eyes and skin, as the substance may cause irritation. Use adequate ventilation when weighing the powder or preparing solutions. Avoid incompatible chemicals, follow approved spill-response and waste-disposal procedures, and ensure appropriate supervision during educational laboratory experiments.