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azamat
2 years ago
6

In a redox reaction, which ion would you expect to be more easily reduced? In a redox reaction, which ion would you expect to be

more easily reduced? Hypochlorite ion, ClO− They are equally reducible. Not enough information is given. Perchlorate, ClO−4
Chemistry
1 answer:
Levart [38]2 years ago
7 0

Answer:

In a redox reaction, hypochlorite ion would be more easily reduced.

Explanation:

Hypochlorite compounds are generally unstable - e.g. sodium hypochlorite is not available in solid form, because removing water from a NaClO disolution, causes a dismutation, turning it in a mixture of NaCl y NaClO3. Heating the same disolutions will also cause this effect. Hypochlorite will decompose under solar light into chlorides and oxygen.

Due to their low stability, hypochlorite compounds (i.e. those containing the hypochlorite ion) are very strong oxidants. Perchlorate ion can balance its negative charge instead and thus will be less prone to reduction than hypochlorite.

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An inorganic substance with the formula BaCl2 is barium chloride. It is one of the most popular barium salts that dissolve in water. Like the majority of other water-soluble barium salts, it is white, extremely hazardous, and gives flames a yellow-green tint.

When 1 mole of bacl2 is dissolved in water it releases-8.67 kj/mil of energy. calculate h when 10.3 g of barium chloride is dissolved to make a 1.00 l solution

In water, barium chloride is very soluble (as is the case with most ionic salts). In its dissolved condition, it is known to split into barium cations and chloride anions.

Let's first determine the total amount of CL- ions.

=> When HCl dissociates, one mol will produce H+ and one mol will produce CL-. Thus, . 2 moles yields. 2 mol CL-

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= .4/.5 = 0.8 M

As a result, 0.8 M is the molarity of CL- in solution.

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