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Consulting Table 3.1, arrange the follow...

Consulting Table 3.1, arrange the following species in order of increaing stregth as oxidizing agents: `MnO_(4)^(-)` (in acidic solution) `Sn^(+)`, `Al^(3+)`, `Co^(3+)`, and `Ag^(+)`. Assume all species are in their standard states.

A

`Al^(3+) lt Sn^(2+) lt Ag^(+) lt MnO_(4)^(-) gt Co^(3+)`

B

`Al^(3+) lt Sn^(2+) lt Ag^(+) lt Co^(3+) gt MnO_(4)^(-)`

C

`Al^(3+) ltSn^(2+) lt Co^(3+) lt Ag^(+) gt MnO_(4)^(-)`

D

`Al^(3+) lt Co^(2+) lt Sn^(3+) lt Ag^(+) gt MnO_(4)^(-)`

Text Solution

Verified by Experts

The correct Answer is:
A
Using Table 3.1, we write the half-reactions in the order in which they appear there:
`Al^(3+)(aq., 1 M)+3e^(-) underset(larr)(rarr) Al(s) E^(@) = -1.66 V`
`Sn^(2+)(aq., 1 M)+2e^(-) underset(larr)(rarr) Sn(s) E^(@) = -0.14 V`
`Ag^(2)(aq.,1M)+e^(-)hArr Ag(s)E^(@)=0.80 V`
`MnO_(4)^-)(aq.,1M)+8H^(+)(aq.,1M)+5e^(-)hArr Mn^(2-) (aq.,1M)+4H_(2)O(1)E^(@) = 1.51V`
`Co^(3+)(aq.,1M)+e^(-)hArr Co^(2+)(aq.,1M)E^(@)=1.82V`
Oxidizing agent oxidizes the other and gets reduced. Thus, strength of an oxidizing agent is directly related to its reduc-tion potential i.e. the more positive the standard reducation potential, the greater the tendency of the species to be reduced or the stronger the species as an oxidizing agent. Thus the oxidizing agents increases in strength with the increases of reduction potential as follows:
`Al^(3+),Sn^(2+) lt Ag^(+) lt MnO_(4)^(-) lt Co^(3+)`
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