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Chapter 9: Problem 23

The reaction of slaked lime with \(\mathrm{Cl}_{2}\) gas gives: (a) A mixture of \(\mathrm{Ca}(\mathrm{OCl})_{2}, \mathrm{Ca}(\mathrm{OH})_{2}, \mathrm{CaCl}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) (b) Quick lime (c) Baryta water (d) Only \(\mathrm{Ca}(\mathrm{OCl})_{2}\)

Short Answer

Expert verified
The correct answer is (a).

Step by step solution

01

Understanding the Chemical Reaction

Slaked lime is chemically known as calcium hydroxide \(\mathrm{Ca(OH)_2}\). When slaked lime reacts with chlorine gas \(\mathrm{Cl_2}\), it forms bleaching powder, which is a mixture of compounds, not a single compound.
02

Identify the Expected Products

The reaction between slaked lime and chlorine gas typically results in the formation of bleaching powder, chemically represented as a mixture containing \(\mathrm{Ca(OCl)_2}, \mathrm{Ca(OH)_2}, \mathrm{CaCl_2}\), and water (\(\mathrm{H_2O}\)). This implies multiple products are formed, not just one.
03

Analyzing Each Option

- Option (a) lists the mixture \(\mathrm{Ca(OCl)_2}, \mathrm{Ca(OH)_2}, \mathrm{CaCl_2}\) and water, which matches the products of the reaction.- Option (b) quick lime, known as \(\mathrm{CaO}\), is not a product of this reaction.- Option (c) baryta water, consisting of \(\mathrm{Ba(OH)_2}\) in water, is unrelated to the reactants.- Option (d) suggests only \(\mathrm{Ca(OCl)_2}\) is formed, which is incorrect as other compounds are also produced.
04

Conclusion

Based on the analysis, the correct reaction products are listed in option (a). Therefore, the mixture produced by the reaction is \(\mathrm{Ca(OCl)_2}, \mathrm{Ca(OH)_2}, \mathrm{CaCl_2}\), and water.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Slaked Lime
Slaked lime, also known as calcium hydroxide, is a compound with the chemical formula \(\mathrm{Ca(OH)_2}\). It appears as a white powder or crystal. This chemical is produced by mixing quick lime \(\mathrm{CaO}\) with water, a process called slaking. During slaking, heat is released, and the resulting compound is less aggressive and easier to handle compared to its parent compound, quick lime.
Slaked lime is a key ingredient in various industrial and household applications:
  • Used in the construction industry in mortars and plasters.
  • Important in wastewater treatment as it adjusts pH levels and precipitates impurities.
  • Acts as a neutralizing agent in acidic soil for agriculture.
Its significance extends to chemical reactions, such as its role in the production of bleaching powder when reacted with chlorine gas \(\mathrm{Cl_2}\). Understanding slaked lime is essential for comprehending how it leads to multiple products in such reactions.
Bleaching Powder
Bleaching powder is a white amorphous powder that serves a multitude of purposes in various sectors, primarily due to its effective bleaching and disinfectant properties. Chemically, the compound is often represented as a mixture containing \(\mathrm{Ca(OCl)_2}\), \(\mathrm{Ca(OH)_2}\), and \(\mathrm{CaCl_2}\). The composition results from a reaction of slaked lime \(\mathrm{Ca(OH)_2}\) with chlorine gas \(\mathrm{Cl_2}\).
  • It is widely used in the textile industry for bleaching cotton and linen.
  • In water treatment facilities, it is used to disinfect and treat sewage to ensure safe water quality.
  • As a disinfectant, it kills bacteria, making it valuable in sanitation work.
Bleaching powder, due to its varied components, can serve multiple functions owing to the presence of calcium hypochlorite \(\mathrm{Ca(OCl)_2}\), which contributes significantly to its bleaching action. The versatility of bleaching powder makes it indispensable across multiple industries.
Chlorine Gas Reaction
The reaction of slaked lime \(\mathrm{Ca(OH)_2}\) with chlorine gas \(\mathrm{Cl_2}\) is an important chemical process that produces bleaching powder. This reaction signifies an interesting interplay between an inorganic base and a gas, leading to a solid product mixture.Some important points about this reaction are:
  • The balanced chemical equation for this reaction is: \[2\mathrm{Ca(OH)_2} + 2\mathrm{Cl_2} \rightarrow \mathrm{Ca(OCl)_2} + \mathrm{CaCl_2} + 2\mathrm{H_2O}\]
  • The process involves a substitution reaction where chlorine replaces hydroxyl groups to form calcium hypochlorite.
  • Water is also produced as a byproduct, making this a wet reaction.
Interpreting these reactions provides critical insights into the products formed and the practical applications of these reaction products, namely bleaching powder. Such reactions demonstrate the practical utility of chemistry in producing materials that serve vital purposes in everyday life.

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