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Because H SO s sulfur atom cannot lose any more electrons it cannot be a reducing agent Instead it typically acts as an oxidizing agent gaining electrons and being reduced
If it is reduced in a chemical reaction it will gain electrons The species that loses the electrons has been oxidised and therefore sulfuric acid can be an oxidising agent but never a reducing agent as S
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H 2 S O 4 is a strong oxidizer Since H 2 S O 4 is a strong acid it reacts with a weak amphoteric base water in dilute concentrations to produce H 3 O ions However since the condensed solution is
An oxidizing agent gains electrons and is reduced Sulfur in H 2 SO 4 has an oxidation state of 6 If it decreases H 2 SO 4 is acting as an oxidizing agent If the oxidation state of sulfur remains 6 it is
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In modern terms a reducing agent donates electrons to another substance causing the other substance to be reduced Consequently the reducing agent itself gets oxidised in the chemical
H2SO4 2H SO4 is a redox reaction where O is oxidized and H S are reduced H 2 SO 4 are reducing agents i e they lost electrons and H 2 SO 4 H 2 SO 4 are oxidizing agents i e they
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If it is reduced in a chemical reaction it will gain electrons The species that loses the electrons has been oxidised and therefore sulfuric acid can be an oxidising agent but never a reducing agent as S
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Sulfuric acid H2SO4 is generally known to act as an oxidizing agent due to the high oxidation state of sulfur 6 Being already at the highest stable oxidation state 6 sulfur in H2SO4
If it is reduced in a chemical reaction it will gain electrons The species that loses the electrons has been oxidised and therefore sulfuric acid can be an oxidising agent but never a reducing agent as S
Sulfuric acid H2SO4 is generally known to act as an oxidizing agent due to the high oxidation state of sulfur 6 Being already at the highest stable oxidation state 6 sulfur in H2SO4
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