Problem 6
Question
The products obtained when chlorine gas reacts with cold and dilute aqueous \(\mathrm{NaOH}\) are : [Main 2017] (a) \(\mathrm{ClO}\) and \(\mathrm{ClO}_{3}\) (b) \(\mathrm{ClO}_{2}\) and \(\mathrm{ClO}_{3}\) (c) \(\mathrm{Cl}^{-}\)and \(\mathrm{ClO}^{-}\) (d) \(\mathrm{Cl}^{-}\)and \(\mathrm{ClO}_{2}\)
Step-by-Step Solution
Verified Answer
The products are \(\mathrm{Cl}^-\) and \(\mathrm{ClO}^-\) (option c).
1Step 1: Write the Reaction Equation
When chlorine gas reacts with cold, dilute aqueous sodium hydroxide (\(\mathrm{NaOH}\)), the reaction can be expressed as follows: \[ \mathrm{Cl_2 + 2NaOH \rightarrow NaCl + NaClO + H_2O} \]In this reaction, chlorine gas reacts with sodium hydroxide to produce sodium chloride (NaCl), sodium hypochlorite (NaClO), and water (H₂O).
2Step 2: Identify the Products
From the balanced equation, we can see that the products are \(\mathrm{NaCl}\), \(\mathrm{NaClO}\), and water (\(\mathrm{H_2O}\)). In terms of ions, the products are \(\mathrm{Cl}^-\) from sodium chloride and \(\mathrm{ClO}^-\) from sodium hypochlorite.
3Step 3: Match the Reaction Products with Answer Choices
Now compare the obtained products from the reaction: \(\mathrm{Cl}^-\) (from \(\mathrm{NaCl}\)) and \(\mathrm{ClO}^-\) (from \(\mathrm{NaClO}\)) with the given options.The correct answer matches with option (c) \(\mathrm{Cl}^-\) and \(\mathrm{ClO}^-\).
Key Concepts
Chlorine ChemistryAqueous SolutionsChemical Reactions
Chlorine Chemistry
Chlorine (\( \mathrm{Cl_2} \)) is a yellow-green gas belonging to the halogen group in the periodic table. Halogens are known for their reactivity, and chlorine is no exception. Its behavior in reactions can vary widely depending on the conditions, such as temperature and the presence of other chemicals. In the reaction with sodium hydroxide (\( \mathrm{NaOH} \)), chlorine undergoes a fascinating transformation. When chlorine gas comes into contact with cold, dilute aqueous \( \mathrm{NaOH} \), it reacts to form both sodium chloride (\( \mathrm{NaCl} \)) and sodium hypochlorite (\( \mathrm{NaClO} \)). This is an example of a disproportionation reaction, where chlorine is simultaneously reduced and oxidized.
It's important to note that chlorine doesn't always react this way. For instance, when reacting with hot sodium hydroxide, chlorine forms different products, such as sodium chloride and sodium chlorate (\( \mathrm{NaClO_3} \)). Understanding chlorine's chemistry is crucial because it's used extensively in industry, especially in water treatment and the manufacture of bleaching agents.
It's important to note that chlorine doesn't always react this way. For instance, when reacting with hot sodium hydroxide, chlorine forms different products, such as sodium chloride and sodium chlorate (\( \mathrm{NaClO_3} \)). Understanding chlorine's chemistry is crucial because it's used extensively in industry, especially in water treatment and the manufacture of bleaching agents.
Aqueous Solutions
An aqueous solution is simply a solution in which water is the solvent. Water's unique properties make it an excellent solvent for many substances. In the case of \( \mathrm{NaOH} \) in the reaction with chlorine gas, the \( \mathrm{NaOH} \) is dissolved in water, allowing it to mix thoroughly with the chlorine gas. This aqueous environment is key for the reaction to occur efficiently.
The ions in aqueous solutions, such as \( \mathrm{Na^+} \) and \( \mathrm{Cl^-} \), are free to move, facilitating the reaction process. The water molecules stabilize these ions, making interactions between them possible. When handling solutions like these, especially when they involve reactive elements like chlorine, safety is very important. Chlorine solutions are often used for their disinfecting properties, but they should be handled with care due to their potential hazards.
The ions in aqueous solutions, such as \( \mathrm{Na^+} \) and \( \mathrm{Cl^-} \), are free to move, facilitating the reaction process. The water molecules stabilize these ions, making interactions between them possible. When handling solutions like these, especially when they involve reactive elements like chlorine, safety is very important. Chlorine solutions are often used for their disinfecting properties, but they should be handled with care due to their potential hazards.
Chemical Reactions
In chemistry, reactions describe how substances interact to form new products. The reaction between chlorine gas and cold, dilute aqueous sodium hydroxide is a classic example of a chemical reaction, specifically a redox reaction. In this process, electrons are transferred between substances.
During this reaction, chlorine gas interacts with the sodium hydroxide solution to form products like \( \mathrm{NaCl} \) and \( \mathrm{NaClO} \). The reaction can be written as:\[\mathrm{Cl_2 + 2NaOH \rightarrow NaCl + NaClO + H_2O}\]This equation shows that each chlorine molecule reacts with two sodium hydroxide molecules to produce sodium chloride, sodium hypochlorite, and water.
Key points to note include:
During this reaction, chlorine gas interacts with the sodium hydroxide solution to form products like \( \mathrm{NaCl} \) and \( \mathrm{NaClO} \). The reaction can be written as:\[\mathrm{Cl_2 + 2NaOH \rightarrow NaCl + NaClO + H_2O}\]This equation shows that each chlorine molecule reacts with two sodium hydroxide molecules to produce sodium chloride, sodium hypochlorite, and water.
Key points to note include:
- Chlorine is both oxidized and reduced – a hallmark of disproportionation reactions.
- The reaction is balanced, showing the conservation of atoms and charge.
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