Why is the oxidation of #Mn^(2+)# in ACIDIC media represented differently to the oxidation of #Mn^(2+)# in an ALKALINE medium? What do we mean by #H^+# or #H_3O^+#?

Answer 1

Because chemistry follows experiment...........

#H^+# is very much a conceptual particle. When we write #H^+# in a reaction we mean the hydronium ion, #H_3O^+#, which AGAIN is a conceptual species. The actual species is (probably) a cluster of 3-4 water molecules, with an extra proton to give #H_7O_3^+#, or #H_9O_4^+#. The clusters exchange the proton between themselves. We write #H^+# or #H_3O^+# for convenience.
When we write a redox equation, of course we balance mass and charge, and the use of #H^+# or #H_3O^+# is a means to this end. It happens that in ACIDIC medium, #Mn^(2+)#, may be oxidized to #MnO_4^(-)#:
#Mn^(2+) +4H_2O rarr MnO_4^(-) + 8H^(+) + 5e^-#
In alkaline media, #Mn^(2+)# may be oxidized to #"manganate ion"#, #MnO_4^(2-)#, which is #Mn(VI+)#:
#Mn^(2+) +8HO^(-) rarr MnO_4^(2-) + 4H_2O + 4e^-#

Green salts are given by "manganates".

It should be noted that this representation follows the actual experiment, not the other way around. Mass and charge are balanced (I believe) as required.

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Answer 2

The oxidation of Mn^(2+) in acidic media is represented differently from the oxidation of Mn^(2+) in alkaline media because in acidic conditions, the reaction involves the formation of MnO2 (manganese dioxide), whereas in alkaline conditions, the reaction produces MnO4^2- (permanganate ion).

H^+ or H3O^+ represent positively charged hydrogen ions, also known as hydronium ions. They are formed when a hydrogen ion (H^+) combines with a water molecule (H2O) to form a hydronium ion (H3O^+).

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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