0.2 mol of Na₃PO₄ and 0.5 mol of Ba(NO₃)₂ are mixed in 1L of solution. Which of the following is/ are correct about this system?

$2{\mathrm{Na}}_3{\mathrm{PO}}_4\left(\mathrm{aq}\right)+3\mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2\left(\mathrm{aq}\right)⟶{\mathrm{Ba}}_3{\left({\mathrm{PO}}_4\right)}_2\left(\mathrm{s}\right)+6{\mathrm{NaNO}}_2\left(\mathrm{aq}\right)$

Na₃PO₄ is the limiting reactant and is completely consumed.

$\text{ Mol of }{\mathrm{Ba}}_3{\left({\mathrm{PO}}_4\right)}_2\text{ formed }=\frac{0.2}{2}=0.1\text{; }$

$\text{ mol of }\mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2\text{ reacted }=\frac{3}{2}\times 0.2=0.3$

Mol of unreacted Ba(NO₃)₂ = 0.5 - 0.3=0.2  moL of Ba²⁺ ion

Mol of Na⁺ in solution = 0.2 × 3 = 0.6;
Mol of NO₃ ^- in solution = 0.5 × 2 = 1.