Question

Use oxidation states to identify the element/ion that is oxidized and the element/ion that is reduced,...

Use oxidation states to identify the element/ion that is oxidized and the element/ion that is reduced, as well as the oxidizing and reducing agent in the following redox reaction.

Ba(s) + 2HCl(aq) --> BaCl2(aq) + H2(g)

being oxidized:

being reduced:

oxidizing agent:

reducing agent:

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Answer #1

Given redox reaction is,

Ba(s) + 2HCl(aq) BaCl2(aq) + H2(g)

oxidation state of Ba(s) = 0

oxidation state of hydrogen ion in HCl (aq) = +1

oxidation state of chloride ion in HCl (aq) = -1

oxidation state of Barium ion in BaCl2(aq) = +2 [ x-2 = 0; x=2]

oxidation state of chloride ion in BaCl2(aq) = -1 [no change]

oxidation state of hydrogen in H2(g) = 0

from this calculation we can see that Barium changes oxidation state from 0 to +2

i.e gets oxidised by loosing electrons.

Such element loosing electrons in the redox reaction is said to be reducing agent.

Also hydrogen changes oxidation state from +1 to 0.

i.e. gets reduced by gaining electrons.

the element gaining electrons in the redox reaction is said to be oxidising agent.

Hence, in the given reaction,

being oxidised : Ba

being reduced: HCl

oxidizing agent: HCl

Reducing agent: Ba

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