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Iodic acid is a white water-soluble solid with the chemical formula HIO 3.Its robustness contrasts with the instability of chloric acid and bromic acid.Iodic acid features iodine in the oxidation state +5 and is one of the most stable oxo-acids of the halogens.
The conjugate base is hypoiodite (IO −). Salts of this anion can be prepared by treating iodine with alkali hydroxides. They rapidly disproportionate to form iodides and iodates, [2] but an iodine–hydroxide mixture can be used an in situ preparation of hypoiodite for other reactions. [3]
Hydrogen iodide (HI) is a diatomic molecule and hydrogen halide. Aqueous solutions of HI are known as hydroiodic acid or hydriodic acid, a strong acid.Hydrogen iodide and hydroiodic acid are, however, different in that the former is a gas under standard conditions, whereas the other is an aqueous solution of the gas.
On the other hand, if a chemical is a weak acid its conjugate base will not necessarily be strong. Consider that ethanoate, the conjugate base of ethanoic acid, has a base splitting constant (Kb) of about 5.6 × 10 −10, making it a weak base. In order for a species to have a strong conjugate base it has to be a very weak acid, like water.
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Iodate is one of several oxyanions of iodine, and has an oxidation number of +5. It participates in several redox reactions, such as the iodine clock reaction.Iodate shows no tendency to disproportionate to periodate and iodide, in contrast to the situation for chlorate.
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Its conjugate base is the acetate ion with K b = 10 −14 /K a = 5.7 x 10 −10 (from the relationship K a × K b = 10 −14), which certainly does not correspond to a strong base. The conjugate of a weak acid is often a weak base and vice versa.