A `0.025M` solution of a monobasic acid had a freezing point of `-0.06^(@)C`. Calculate `K_(a)` for the acid . `K_(f)(H_(2)O)=1.86`

Explanation

To solve the problem of calculating the dissociation constant \( K_a \) for a monobasic acid from the given information, we will follow these steps:

### Step 1: Understand the given data
- Molarity of the acid solution, \( C = 0.025 \, M \)
- Freezing point depression, \( \Delta T_f = -0.06^\circ C \)
- Cryoscopic constant of water, \( K_f = 1.86 \, \text{°C kg/mol} \)

### Step 2: Calculate the freezing point depression
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