When a 0.1 N solution of a monoprotonic acid at room temperature has a degree of ionization of 10%, the concentration of hydroxyl ions in g ion/litre would be

To determine the concentration of hydroxyl ions \(\text{OH}^-\) in a 0.1 N solution of a monoprotonic acid with a degree of ionization of 10%, let's break down the steps:

1. **Degree of Ionization**: 
   - The degree of ionization \(\alpha\) is given as 10%, which is 0.1 in decimal form.

2. **Concentration of Hydrogen Ions \([\text{H}^+]\)**:
   - Since the acid is monoprotonic (i.e., it donates one proton per molecule), the concentration of \(\text{H}^+\) ions will be:
     \[
     [\text{H}^+] = \alpha \times C = 0.1 \times 0.1 \, \text{N} = 0.01 \, \text{N}
     \]

3. **Determination of \([\text{OH}^-]\)**:
   - At room temperature, we assume \(T = 25^\circ C\), and the ionic product of water \(K_w\) is \(1 \times 10^{-14}\) mol\(^2\) L\(^{-2}\).
   - The concentration of hydroxyl ions \([\text{OH}^-]\) can be determined using the relation:
     \[
     [\text{OH}^-] = \frac{K_w}{[\text{H}^+]} = \frac{1 \times 10^{-14}}{0.01} = 1 \times 10^{-12} \, \text{mol/L}
     \]

4. **Conversion to g ion/L**:
   - Since the concentration is required in \(g \, \text{ion/L}\), and the molecular weight of \(\text{OH}^-\) is approximately 17 g/mol:
     \[
     [\text{OH}^-] \text{ in g ion/L} = 1 \times 10^{-12} \, \text{mol/L} \times 17 \, \text{g/mol} = 1.7 \times 10^{-11} \, \text{g ion/L}
     \]

**Final Answer**: The concentration of hydroxyl ions in the solution is \(1.7 \times 10^{-11}\) g ion/L.

Would you like more details on any step or have further questions?

Here are some related questions:
1. What is the significance of the degree of ionization in weak acids?
2. How does temperature affect the ionic product of water (\(K_w\))?
3. What factors influence the degree of ionization in acids?
4. How would the concentration of \([\text{OH}^-]\) change if the degree of ionization was increased?
5. What is the relationship between the normality and molarity of a monoprotonic acid?

**Tip**: Always remember to verify the units when performing calculations, especially when switching between molar and gram ion concentrations.

Calculate the concentration of hydroxyl ions in a 0.1 N solution of a monoprotonic acid with a 10% degree of ionization. Understand the chemistry behind ionization, acid-base equilibrium, and the calculation steps involved. Suitable for high school chemistry students.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation