One litre of 2 molar solution of a complex salt $CoC{l}_3.4N{H}_3$ (Mol. wt = 233.5) shows an osmotic pressure of 98.40 atm at 300 K. The solution is now treated with 2 litre of 1M $AgN{O}_3.$ Which of the following is/are correct? [Ag = 108] (R = 0.082 L–atm/K–mol)

$CrC{l}_3.6H_{2}O, \pi =iCRTi=1+\alpha (n-1)$

$98.4=i\times 2\times 0.082\times 300, i=2$

$1+\alpha (n-1)=2, 1+n-1=2(\alpha =1), n=2$

$CoC{l}_3.4N{H}_{3}canbewrittenas$ $\left[Co{\left(N{H}_3\right)}_{4}C{l}_2\right]Cl\to {\left[Co{\left(N{H}_3\right)}_{4}C{l}_2\right]}^{\oplus }+C{l}^{(-)}$

$\frac{\begin{array}{l}C{l}^{(-)}+A{g}^{(+)}\to AgCl\downarrow \\ \left(AgN{O}_3\right)\end{array}}{\left[Co{\left(N{H}_3\right)}_{4}Cl\right]Cl+A{g}^{\oplus }\to AgCl+{\left[Co{\left(N{H}_3\right)}_{4}C{l}_2\right]}^{\oplus }}$

$weightofAgCl=2\times 143.5=287g$

$finalsolution=2mole\left[Co{\left(N{H}_3\right)}_{4}C{l}_2\right]N{O}_3$

$totalvolume=1+2=3litre$

$C=\frac{2}{3}$

$$\begin{gathered} \pi =iCRT i=1+\alpha (n-1) \\ =2\times \frac{2}{3}\times 0.082\times 300 =1+\alpha (2-1) \\ \pi =32.8atm =1+\alpha =1+1 \\ i=2 \end{gathered}$$