Question

The compound whose \(0.1 \mathrm{M}\) solution is basic is: (a) Ammonium acetate (b) Ammonium sulphate (c) Sodium acetate (d) Ammonium chloride

Short answer

The compound with a basic solution is sodium acetate (c).

Step-by-step solution

Understand the Problem

We are asked to identify out of four compounds which one results in a basic solution at a concentration of \(0.1 \text{ M}\). A basic solution will have a pH greater than 7, indicating the presence of OH\(^-\) ions.

Analyze the Compounds

Analyze each compound's dissociation in water:1. **Ammonium acetate:** \( \text{NH}_4\text{CH}_3\text{COO} \) dissociates into \( \text{NH}_4^+ \) (acidic) and \( \text{CH}_3\text{COO}^- \) (basic) ions.2. **Ammonium sulphate:** \( \text{(NH}_4\text{)}_2\text{SO}_4 \) dissociates into \( \text{NH}_4^+ \) (acidic) and \( \text{SO}_4^{2-} \) ions.3. **Sodium acetate:** \( \text{CH}_3\text{COONa} \) dissociates into \( \text{Na}^+ \) and \( \text{CH}_3\text{COO}^- \) (basic) ions.4. **Ammonium chloride:** \( \text{NH}_4\text{Cl} \) dissociates into \( \text{NH}_4^+ \) (acidic) and \( \text{Cl}^- \) ions.

Identify the Basic Ions

Identify the ions that contribute to a basic solution:- **Ammonium ion (\( \text{NH}_4^+ \))** is an acidic ion.- **Acetate ion (\( \text{CH}_3\text{COO}^- \))** is a basic ion.- **Sodium ion (\( \text{Na}^+ \)) and Chloride ion (\( \text{Cl}^- \))** are neutral.

Determine the Compound Creating a Basic Solution

The sodium acetate produces the basic ion \( \text{CH}_3\text{COO}^- \) without any accompanying acidic ion, resulting in a basic solution.\(\text{Sodium acetate} \rightarrow \text{CH}_3\text{COO}^- + \text{Na}^+ \)

Conclusion

The compound whose \(0.1 \text{ M}\) solution is basic is **sodium acetate**.

Key concepts

Sodium Acetate

Sodium acetate is a fascinating compound that can be found in your everyday life, like when you use it in heat packs or in the food industry as a seasoning. Chemically, sodium acetate is known by its formula \( \text{CH}_3\text{COONa} \). This compound has a unique behavior when mixed into a solution, particularly in water, which we'll explore further below.

When dissolved in water, sodium acetate dissociates into two ions: the sodium ion (\( \text{Na}^+ \)) and the acetate ion (\( \text{CH}_3\text{COO}^- \)).

• The sodium ion is generally neutral and doesn't impact the pH of the solution.
• The acetate ion, however, acts as a base and can influence the pH to make the solution basic.

This property is essential in various fields, especially in studies concerning chemical reactions where knowing whether a solution is acidic or basic is crucial.

Compound Dissociation in Water

Understanding how compounds dissociate in water helps identify their roles in creating solutions with specific properties. Dissociation refers to the process where molecules split into smaller particles, typically ions, when in a solution.

Take sodium acetate, for instance. In water, it dissociates seamlessly into acetate ions (\( \text{CH}_3\text{COO}^- \)) and sodium ions (\( \text{Na}^+ \)). Other compounds dissociate differently:

• Ammonium acetate results in both the acidic ion \( \text{NH}_4^+ \) and the basic ion \( \text{CH}_3\text{COO}^- \).
• Ammonium sulphate results in acidic \( \text{NH}_4^+ \) and sulphate ions \( \text{SO}_4^{2-} \) that don't significantly affect the solution's pH.
• Ammonium chloride dissociates into \( \text{NH}_4^+ \) (acidic) and \( \text{Cl}^- \) ions, which are neutral in effect.

By evaluating how each compound dissociates, chemists can predict their roles when mixed into water, aiding in determining their use in various applications, from industrial solutions to educational purposes.

Acidic and Basic Ions Identification

In the world of chemistry, identifying whether an ion is acidic or basic is central to predicting the outcome of reactions and the nature of solutions. An acidic ion donates hydrogen ions to the solution, lowering the pH.

On the flip side, basic ions like acetate (\( \text{CH}_3\text{COO}^- \)) tend to remove hydrogen ions from the solution, thus increasing the pH and making it more basic. Here is what you generally observe in ions:

• Acetic ions such as \( \text{NH}_4^+ \) in ammonium compounds release \( \text{H}^+ \) and alter the solution to be more acidic.
• Basic ions such as \( \text{CH}_3\text{COO}^- \) have the opposite effect, grabbing \( \text{H}^+ \) ions and making the solution less acidic.
• Neutral ions, like \( \text{Na}^+ \) and \( \text{Cl}^- \), do not necessarily impact the solution's pH as they neither donate nor accept H\(^+\) from the environment.

Understanding these behaviors helps chemists predict and manipulate chemical reactions and can also help in everyday applications like managing water pH or formulating chemical solutions for different uses.