Is this reaction a redox reaction? Is there any change in oxidation numbers?
Aluminium nitrate + concentrated sulfuric acid
I heard that concentrated sulfuric acid acts differently from the dilute acid. What are the properties of the concentrated acid?
2007-04-09 00:33:46 · 3 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
I don't think there is any reaction.
Concentrated sulfuric acid is different from the dilute acid in that it acts as an oxidising agent. For example, it reacts with copper metal to form sulfur dioxide.
However, note that basically all acids would be oxidising agents because proton reacts with many metals to form the metal ions and hydrogen gas.
nH(+) + M(s) = (n/2)H2(g) + M(n+)
Thus, when we describe the redox properties of acids, we focus on the possible change of the oxidation state of the non-hydrogen elements (i.e. sulfur in this case).
Since Al(NO3)3 is not redox-active, I don't think there is any chemical reaction when conc H2SO4 is added. However, the temperature of the solution would become higher and there may be some acid vapour evolved (as suggested in another answer).
2007-04-09 02:25:07 · answer #1 · answered by cccccrazy 2 · 0⤊ 0⤋
My prediction for this rather unusual reaction would be that it would release nitric acid vapour through an acid displacement reaction, leaving aluminium sulphate. It's very similar to the old laboratory preparation of nitric acid, and it is not redox.
2007-04-09 01:21:31 · answer #2 · answered by Gervald F 7 · 0⤊ 0⤋
No - there are no charge changes. The sulfur in SO2 = +4 The sulfur in H2SO3 = +4 H is +1 in H20 and H2SO3, O is -2 is H20 ahd H2SO3 This is a synthesis reaction
2016-05-20 22:32:04 · answer #3 · answered by ? 3 · 0⤊ 0⤋