Question

Hydrogen peroxide can not: (a) Give silver peroxide with moist silver oxide (b) Turn the mixture of aniline, \(\mathrm{KClO}_{3}\) and dil. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) violet (c) Liberate iodine from \(\mathrm{KI}\) (d) Turn the titanium salt yellow

Short answer

(b) Turn the mixture of aniline, \(\mathrm{KClO}_3\) and dil. \(\mathrm{H}_2\mathrm{SO}_4\) violet

Step-by-step solution

Analyze Option (a)

Hydrogen peroxide reacts with moist silver oxide to form silver peroxide. The reaction involves the decomposition of hydrogen peroxide where it acts as an oxidizing agent. Hence, option (a) is a reaction that can occur.

Analyze Option (b)

Hydrogen peroxide does not turn a mixture of aniline, \(\mathrm{KClO}_3\), and dilute \(\mathrm{H}_2\mathrm{SO}_4\) violet. Instead, it's oxidation of the compound that gives the color. Therefore, this reaction is not characteristic of hydrogen peroxide.

Analyze Option (c)

Hydrogen peroxide can act as an oxidizing agent and liberate iodine from \(\mathrm{KI}\) as it causes the oxidation of \(\mathrm{I}^-\) to \(\mathrm{I}_2\). Hence, this option is viable.

Analyze Option (d)

Hydrogen peroxide can react with titanium salts to form a yellow-colored titanium-hydrogen peroxide complex. Therefore, it can turn the titanium salt yellow.

Key concepts

Oxidizing Agents

Hydrogen peroxide is a classic example of an oxidizing agent. Chemical substances that trigger the loss of electrons in other substances are called oxidizing agents.
In simpler terms, they give oxygen or accept electrons during a chemical reaction. Hydrogen peroxide oxidizes various substances, which means it takes electrons away from them. This results in the other substance being oxidized, while the oxidizing agent itself gets reduced.
Hydrogen peroxide's role as an oxidizing agent is why it can decompose substances like moist silver oxide to form silver peroxide. It helps facilitate many important chemical reactions by changing the oxidation states of the molecules involved.
Here are some key points about oxidizing agents:

• They are crucial in redox reactions where one substance is oxidized, and the oxidizing agent is reduced.
• They increase the oxygen levels or decrease the hydrogen levels in a compound.
• Common examples include hydrogen peroxide, potassium permanganate, and nitric acid.

Silver Peroxide

Silver peroxide is a compound formed when hydrogen peroxide reacts with moist silver oxide. When hydrogen peroxide breaks down, it releases oxygen, which bonds with silver oxide tomake silver peroxide. This shows how effective hydrogen peroxide is as an oxidizing agent because it facilitates the formation of new compounds.
Silver peroxide is known for its unique properties:

• It appears dark brown in color.
• Possesses oxidizing properties itself.
• Less common than other types of peroxides, it has specialized uses in certain chemical reactions.

The formation of silver peroxide from hydrogen peroxide is a clear demonstration of how critical oxidizing agents can be in the synthesis of new chemical substances.

Iodine Liberation

Iodine liberation occurs when hydrogen peroxide acts on potassium iodide ( KI ). This reaction demonstrates hydrogen peroxide's capacity to instigate changes by oxidizing iodide ions to iodine.
The reaction typically proceeds as follows: hydrogen peroxide oxidizes the I ^- to form I 2 , liberating iodine in the process. This is a reversible process and more complex reactions can occur, but the essence is that an oxidizing agent helps to free iodine from its ionic bonds.
The reaction with KI reveals the impactful role of hydrogen peroxide in aiding the release of iodine:

• It acts as the oxidizing agent facilitating the liberation process.
• Visible as a brownish hue when iodine is freed.

It's important because iodine can be used as an indicator in various chemical processes due to its distinctive appearance when liberated.

Titanium-Hydrogen Peroxide Complex

The titanium-hydrogen peroxide complex is a striking example of the interesting reactions hydrogen peroxide can have with metal salts. When hydrogen peroxide mixes with titanium salts, it forms a yellow-colored compound known as a titanium-hydrogen peroxide complex.
This color change is the result of the bonding interactions between hydrogen peroxide and the titanium ions.
This demonstration reveals hydrogen peroxide's oxidative capabilities as it forms a stable, colored complex with the metal.
Some highlights of this complex include:

• Used to indicate the presence of titanium.
• Provides a visual representation of a chemical reaction with everyday implications.
• Shows the versatility of hydrogen peroxide as a chemical reactant.

In essence, the formation of this complex underscores the diverse reactivity and applications of hydrogen peroxide in analytical chemistry.