Consider the following compounds
$\mathrm{P}:\left[\mathrm{Cr}{\left({\mathrm{H}}_2\mathrm{O}\right)}_4{\mathrm{Cl}}_2\right]\mathrm{Br}\cdot 2{\mathrm{H}}_2\mathrm{O}$ $\mathrm{Q}:\left[\mathrm{Cr}{\left({\mathrm{H}}_2\mathrm{O}\right)}_4{\mathrm{Br}}_2\right]\mathrm{Cl}.2{\mathrm{H}}_2\mathrm{O}$
$\mathrm{R}:\left[\mathrm{Cr}{\left({\mathrm{H}}_2\mathrm{O}\right)}_5\mathrm{Cl}\right]{\mathrm{Br}}_2{\mathrm{H}}_2\mathrm{O}$ $\mathrm{S}:\left[\mathrm{Cr}{\left({\mathrm{H}}_2\mathrm{O}\right)}_6\right]{\mathrm{Cl}}_3$
The false statements regarding these compounds is/are

P and Q are ionization isomers

P and R are hydrate isomers

Given volume of solution of most conducting solution will require (1/3)^rd volume of equimolar AgNO₃ solution for complete precipitation.

2.0 g of R dissolved in 2 litre water will show higher conductance compared with 2.0 g of Q in 2 litre solution