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From a microbial standpoint, the presence of natural chlorate could also explain why there is a variety of microorganisms capable of reducing chlorate to chloride. Further, the evolution of chlorate reduction may be an ancient phenomenon as all perchlorate reducing bacteria described to date also utilize chlorate as a terminal electron acceptor ...
Potassium chlorate is the inorganic compound with the molecular formula KClO 3. In its pure form, it is a white solid. After sodium chlorate, it is the second most common chlorate in industrial use. It is a strong oxidizing agent and its most important application is in safety matches. [6]
Potassium perchlorate in crystal form. Potassium perchlorate is prepared industrially by treating an aqueous solution of sodium perchlorate with potassium chloride.This single precipitation reaction exploits the low solubility of KClO 4, which is about 1/100 as much as the solubility of NaClO 4 (209.6 g/100 mL at 25 °C).
The PPIC reported enrollment at California’s most selective public university, the UC, increased by 2% while enrollment declined at California State Universities and community colleges between ...
A perchlorate is a chemical compound containing the perchlorate ion, ClO − 4, the conjugate base of perchloric acid (ionic perchlorate).As counterions, there can be metal cations, quaternary ammonium cations or other ions, for example, nitronium cation (NO + 2).
Tertiary amines can react with DCM to form quaternary chloromethyl chloride salts via the Menshutkin reaction. [22] Secondary amines can react with DCM to yield an equilibrium of iminium chlorides and chloromethyl chlorides, which can react with a second equivalent of the secondary amine to form aminals . [ 23 ]
The State of California Franchise Tax Board (FTB) explained on its website that if you are eligible, you will automatically receive a payment — which is expected to be issued between October ...
The chlorite ion adopts a bent molecular geometry, due to the effects of the lone pairs on the chlorine atom, with an O–Cl–O bond angle of 111° and Cl–O bond lengths of 156 pm. [1] Chlorite is the strongest oxidiser of the chlorine oxyanions on the basis of standard half cell potentials.