Potassium chloride
CAS number:7447-40-7
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Molecular Formula:
ClK
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Molecular Weight:
74.55g/mol
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Brief Introduction:
Potassium chloride (KCl) has been extensively studied for its applications in various fields, including glass modification, radiotherapy dosimetry, and ion-pair recognition. In the context of tellurite glass modification, KCl was found to significantly influence the thermal stability, optical properties, and gamma shielding effectiveness of the glass system. As the KCl concentration increased, the glass transition temperature decreased, while the optical energy gap and thermal stability increased. The addition of KCl also enhanced the gamma shielding properties of the glass, making it a suitable candidate for shielding and optical applications. In radiotherapy, KCl was shown to improve the dose sensitivity of N-(Hydroxymethyl)acrylamide (NHMA) polymer gel dosimeters by up to 33% at a concentration of 1.9 wt%, with the dosimeter exhibiting stability within 2–120 hours post-irradiation. Furthermore, in the realm of molecular recognition, a chalcogen-bonding heteroditopic receptor was designed to selectively recognize KCl over other alkali metal chlorides through a unique ion-pair binding mechanism, demonstrating significant potential for applications in ion channel regulation and cancer treatment.
Salts
KCl is an ionic compound formed from the neutralization reaction between a strong acid (hydrochloric acid, HCl) and a strong base (potassium hydroxide, KOH). It consists of potassium ions (K⁺) and chloride ions (Cl⁻) held together by ionic bonds.
Inorganic Compounds
KCl is classified as an inorganic compound because it does not contain carbon-hydrogen (C-H) bonds, which are characteristic of organic compounds. It is composed of elements other than carbon and hydrogen.
Alkali Metal Halides
KCl is a member of this category because it is composed of potassium (an alkali metal from Group 1 of the periodic table) and chlorine (a halogen from Group 17). Alkali metal halides are known for their high solubility in water and their ability to dissociate into their respective ions.
Electrolytes
KCl dissociates into K⁺ and Cl⁻ ions in aqueous solution, making it an electrolyte. These ions can conduct electricity, which is why KCl is used in various applications requiring ionic conductivity.
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