The experimental van't Hoff factor () for a dilute aqueous solution of Barium nitrate, , is carefull — Solutions and Colligative Properties Chemistry Question
Question
The experimental van't Hoff factor ($i$) for a dilute $0.1\text{ M}$ aqueous solution of Barium nitrate, $Ba(NO_3)_2$, is carefully measured to be exactly $2.74$. What is the percentage degree of dissociation ($\% \alpha$) of the salt?
Answer: A
💡 Solution & Explanation
$Ba(NO_3)_2$ dissociates into 3 ions ($n=3$). Using the relation $\alpha = \frac{i - 1}{n - 1}$, we get $\alpha = \frac{2.74 - 1}{3 - 1} = \frac{1.74}{2} = 0.87$. Multiplying by 100 gives exactly $87\%$.
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