When $0.0106 \text{ mole}$ of acetic acid is dissolved in $1 \text{ kg}$ of water, the observed freezing point depression is $0.0205 \text{ K}$. If the calculated freezing point depression is $0.0197 \text{ K}$, the Van't Hoff factor $(i)$ and the degree of dissociation $(\alpha)$ of acetic acid are respectively:
- A$1.041$ and $0.041$
- B$1.041$ and $0.1041$
- C$0.041$ and $0.041$
- D$0.041$ and $1.041$
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