Analyzing Complex Ion Conductivity
The electrical conductivity of an aqueous solution is directly proportional to the number of ions it contains. For solutions of the same molar concentration ($0.001\text{ M}$), the complex species that dissociates to produce the maximum number of ions will exhibit the highest conductivity.
Dissociation and Ion Formation
Let's analyze the dissociation of each complex in water:
- (i) $[Pt(NH_3)_6]Cl_4$: This complex dissociates into one complex cation and four chloride anions. $[Pt(NH_3)_6]Cl_4 \rightarrow [Pt(NH_3)_6]^{4+} + 4Cl^-$ Total ions formed = $1 + 4 = 5$ ions.
- (ii) $[Cr(NH_3)_6]Cl_3$: This complex dissociates into one complex cation and three chloride anions. $[Cr(NH_3)_6]Cl_3 \rightarrow [Cr(NH_3)_6]^{3+} + 3Cl^-$ Total ions formed = $1 + 3 = 4$ ions.
- (iii) $[Co(NH_3)_4Cl_2]Cl$: This complex dissociates into one complex cation and one chloride anion. $[Co(NH_3)_4Cl_2]Cl \rightarrow [Co(NH_3)_4Cl_2]^+ + Cl^-$ Total ions formed = $1 + 1 = 2$ ions.
- (iv) $K_2PtCl_6$: This ionic compound dissociates into two potassium cations and one complex anion. $K_2PtCl_6 \rightarrow 2K^+ + [PtCl_6]^{2-}$ Total ions formed = $2 + 1 = 3$ ions.
Conductivity Order Determination
The number of ions produced by each solution determines their conductivity order:
| Complex Species | Total Ions Formed |
|---|---|
| (i) $[Pt(NH_3)_6]Cl_4$ | 5 |
| (ii) $[Cr(NH_3)_6]Cl_3$ | 4 |
| (iii) $[Co(NH_3)_4Cl_2]Cl$ | 2 |
| (iv) $K_2PtCl_6$ | 3 |
Based on the number of ions formed, the order of conductivity from lowest to highest is:
(iii) < (iv) < (ii) < (i)
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Important Questions from Inorganic Chemistry
- A chromium complex with a formula $\text{CrCl}_3\cdot 6\text{H}_2\text{O}$ has a spin only magnetic moment value of $3.87 \text{ BM}$ and its solution conductivity corresponds to $1 : 2$ electrolyte. $2.75 \text{ g}$ of the complex solution was initially passed through a cation exchanger. The solution obtained after the process was reacted with excess of $\text{AgNO}_3$. The amount of $\text{AgCl}$ formed in the above process is _____ g. (Nearest integer)
[Given: Molar mass in $\text{g mol}^{-1}$ $\text{Cr} : 52; \text{Cl}: 35.5, \text{Ag}: 108, \text{O}: 16, \text{H}: 1$] - Consider the following reactions :
$\text{NaCl} + \text{K}_2\text{Cr}_2\text{O}_7 + \text{H}_2\text{SO}_4 \rightarrow \text{A} + \text{KHSO}_4 + \text{NaHSO}_4 + \text{H}_2\text{O}$
$\text{A} + \text{NaOH} \rightarrow \text{B} + \text{NaCl} + \text{H}_2\text{O}$
$\text{B} + \text{H}_2\text{SO}_4 + \text{H}_2\text{O}_2 \rightarrow \text{C} + \text{Na}_2\text{SO}_4 + \text{H}_2\text{O}$
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The crystal field splitting energy of $[\text{Co(oxalate)}_3]^{3-}$ complex is '$n$' times that of the $[\text{Cr(oxalate)}_3]^{3-}$ complex. Here '$n$' is ___________. (Assume $\Delta_o >> P$)
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