MCQ
Van’t Hoff factor of $BaCl_2$ in its aqueous solution will be : ($BaCl_2$ is $60\%$ ionized in the solution)
- ✓$1.6$
- B$2.2$
- C$3.6$
- D$4.6$
✓
Answer
Correct option: A.
$1.6$
a
Total volume $=500+1500=2000\, \mathrm{ml}=2\, \mathrm{L}$
Total volume $=500+1500=2000\, \mathrm{ml}=2\, \mathrm{L}$
Moles of $\left[\mathrm{Na}^{+}\right]$ ions $=0.2 \times 0.5=0.1$
Concentration of $\left[\mathrm{Na}^{+}\right]$ ions $=\frac{0.1}{2}=0.05 \,\mathrm{M}$
Moles of $\left[\mathrm{Mg}^{2+}\right]$ ions $=0.4 \times 1.5=0.6$
Concentration of $\left[\mathrm{Mg}^{2+}\right]$ ions
$=\frac{0.6}{2}=0.3\, \mathrm{M}=7.2\, \mathrm{gm} / \mathrm{L}$
Moles of $\left[\mathrm{Cl}^{-}\right]$ ions $=0.2 \times 0.5+2 \times 0.4 \times 1.5$
$=1.3$
Concentration of $[\mathrm{Cl}^-]$ ions $=\frac{1.3}{2}=0.65\, \mathrm{M}$
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