The number of ions present in $2.0 \ L$ of a solution of $0.8 \ M \ K_4[Fe(CN)_6]$ is

The complex ion $[Co(en)_2Br_2]^+$ has two optical isomers. Their correct configurations are:

$CuSO_{4(aq)}$ $\xrightarrow{H_2S \uparrow} M \downarrow$ $\xrightarrow[\text{Excess}]{KCN} N + O$
Then final products $N$ and $O$ are respectively.

The aqueous solution of $CuCrO_4$ is green because it contains

$1\,L, 0.02\,M$ solution of $[Co(NH_3)_5SO_4]Br$ is mixed with $1\,L, 0.02\,M$ solution of $[Co(NH_3)_5Br]SO_4$. The resulting solution is divided into two equal parts $(X)$ and treated with excess $AgNO_3$ solution and $BaCl_2$ solution respectively as shown below:
$1\,L$ Solution $(X) + AgNO_3$ solution (excess) $\rightarrow Y$
$1\,L$ Solution $(X) + BaCl_2$ solution (excess) $\rightarrow Z$
The number of moles of $Y$ and $Z$ respectively are:

Given below are two statements:
Statement-$I$: Hybridisation, shape, and spin-only magnetic moment of $K_{3}[Co(CO_{3})_{3}]$ are $sp^{3}d^{2}$, octahedral, and $4.9 \ BM$ respectively.
Statement-$II$: Geometry, hybridisation, and spin-only magnetic moment values $(BM)$ of the ions $[Ni(CN)_{4}]^{2-}$, $[MnBr_{4}]^{2-}$, and $[CoF_{6}]^{3-}$ respectively are square planar, tetrahedral, octahedral; $dsp^{2}$, $sp^{3}$, $sp^{3}d^{2}$ and $0, 5.9, 4.9$.