Will bromine oxidise iron (II) ions in aq solution

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In summary, bromine is a strong oxidizing agent that readily oxidizes iron (II) ions in an aqueous solution, resulting in the formation of iron (III) ions. This is a redox reaction where bromine gains electrons from iron (II) ions and is reduced itself. This reaction can cause a change in color and pH of the solution. It is a spontaneous reaction due to bromine's higher electronegativity, but it can be reversed by adding a reducing agent.
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I am unsure how to do this question :
Will acidified potassium manganate (VII) oxidise hydrogen sulphide to sulphur in aqueous solution?

Will bromine oxidise iron (II) ions in aq solution ?
Will iodine " " " " " " " ?

any ideas
 
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Start out with an equation then go from there.
 
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I would approach this question by first considering the properties of bromine and iron (II) ions. Bromine is a strong oxidizing agent, meaning it has the ability to accept electrons from other substances in a chemical reaction. Iron (II) ions, on the other hand, are easily oxidized, meaning they readily lose electrons in a chemical reaction.

Based on these properties, it is likely that bromine would be able to oxidize iron (II) ions in aqueous solution. This reaction would result in the formation of iron (III) ions and bromide ions. However, the extent of this oxidation reaction would depend on several factors such as the concentration of bromine and the presence of any other substances that may interfere with the reaction.

Regarding the second question, the use of acidified potassium manganate (VII) suggests that the reaction is being carried out in an acidic environment. In this case, it is possible that hydrogen sulphide could be oxidized to sulfur by the manganate (VII) ions. However, the rate and extent of this reaction would also depend on various factors such as the concentration of manganate (VII) ions, the acidity of the solution, and the presence of any other substances that may affect the reaction.

In conclusion, the ability of bromine and acidified potassium manganate (VII) to oxidize iron (II) ions and hydrogen sulphide respectively in aqueous solution is possible, but the extent of these reactions would depend on various factors and would require further experimentation and analysis.
 

1. Will bromine oxidise iron (II) ions in aq solution?

Yes, bromine is a strong oxidizing agent and will readily oxidize iron (II) ions in an aqueous solution.

2. What is the chemical reaction between bromine and iron (II) ions?

The chemical reaction between bromine and iron (II) ions is a redox reaction, where bromine gains electrons from iron (II) ions and therefore oxidizes them, while being reduced itself.

3. How does the oxidation of iron (II) ions by bromine affect the solution?

The oxidation of iron (II) ions by bromine will result in the formation of iron (III) ions, which can cause a change in color of the solution from clear to yellow or brown. It may also affect the pH of the solution.

4. Is the oxidation of iron (II) ions by bromine a spontaneous reaction?

Yes, the oxidation of iron (II) ions by bromine is a spontaneous reaction because bromine has a higher electronegativity than iron and therefore has a greater tendency to gain electrons and oxidize iron (II) ions.

5. Can the oxidation of iron (II) ions by bromine be reversed?

Yes, the oxidation of iron (II) ions by bromine can be reversed by adding a reducing agent, such as hydrochloric acid or sulfur dioxide, which will reduce the iron (III) ions back to iron (II) ions.

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