Calculate the `H^+` ion concentration in 0.1 M `CH_3COOH` if the degree of dissociation of the acid is 0.0132

Explanation

To calculate the \( H^+ \) ion concentration in a 0.1 M solution of acetic acid (\( CH_3COOH \)) with a degree of dissociation (\( \alpha \)) of 0.0132, we can follow these steps:

### Step 1: Understand the Degree of Dissociation
The degree of dissociation (\( \alpha \)) is defined as the fraction of the initial concentration of the acid that dissociates into ions. For acetic acid, the dissociation can be represented as:
\[ CH_3COOH \rightleftharpoons H^+ + CH_3COO^- \]

### Step 2: Set Up the Initial Concentration
Let the initial concentration of acetic acid be \( C = 0.1 \, M \).

### Step 3: Calculate the Change in Concentration
If \( \alpha \) is the degree of dissociation, then the concentration of \( H^+ \) ions produced can be calculated as:
\[ [H^+] = C \cdot \alpha \]
Substituting the values:
\[ [H^+] = 0.1 \, M \cdot 0.0132 \]

### Step 4: Perform the Calculation
Now, we calculate the \( H^+ \) concentration:
\[ [H^+] = 0.1 \cdot 0.0132 = 0.00132 \, M \]

### Step 5: Conclusion
Thus, the concentration of \( H^+ \) ions in the solution is:
\[ [H^+] = 0.00132 \, M \]