0.1 M solution of urea, at a given temperature, is isotonic with

Options

A. 0.1 M NaCl solution
B. 0.1 M glucose solution
C. 0.02 M KCl solution
D. 0.1 `M BaCl_(2)` solution

Answer

To determine which solution is isotonic with a 0.1 M solution of urea, we need to understand the concept of isotonic solutions and how to compare osmotic pressures.

### Step-by-Step Solution:

1. **Understanding Isotonic Solutions**:
- Isotonic solutions are those that have the same osmotic pressure. This means that the concentration of solute particles in both solutions must be equal.

2. **Identifying Urea**:
- Urea (NH₂CONH₂) is a non-electrolyte, which means it does not dissociate into ions in solution. Therefore, a 0.1 M solution of urea contributes 0.1 moles of solute particles per liter.

3. **Finding an Isotonic Solution**:
- To find a solution that is isotonic with 0.1 M urea, we need to look for another non-electrolyte solution that also has a concentration of 0.1 M.

4. **Analyzing Options**:
- If we consider common solutes:
- **Glucose (C₆H₁₂O₆)**: This is also a non-electrolyte and does not dissociate in solution. Therefore, a 0.1 M solution of glucose will also have 0.1 moles of solute particles per liter, making it isotonic with the 0.1 M urea solution.
- **NaCl**: This is a strong electrolyte and dissociates into two ions (Na⁺ and Cl⁻) in solution. A 0.1 M NaCl solution would produce 0.2 moles of solute particles per liter, which means it would not be isotonic with the 0.1 M urea solution.

5. **Conclusion**:
- The 0.1 M solution of urea is isotonic with a 0.1 M solution of glucose.

### Final Answer:
A 0.1 M solution of urea is isotonic with a 0.1 M solution of glucose.