A complex containing `K,Pt(IV)` and `Cl^(-)` is `100%` ionized giving `i=3` the complext is

A complex containing K^(+),Pt(IV) and Cl^(--) is 100% ionised giving i=3 . Thus, complex is:

A complex containing K^(+),Pt(IV) and Cl^(--) is 100% ionised giving i=3 . Thus, complex is:

A complex containing K^(+) , Pt(IV) and Cl^(-) is 100% ionised giving i=3 . Thus , complex is :

A complex iron and cyanide ions is 100% ionised at 1 m (molal) . If its elevation in b.p is 2.08 . Then the complex is (K_(b)=0.52^(@) mol^(-1) kg) :

A complex of iron and cyanide ions is 100% ionised at 1m (mol). If its elevation in b.p is 2.8^(0) , ( K_(b)=0.52^(0) "mol"^(-1)Kg ), then the complex is :

CaCl_(3), xNH_(3) is a complex compound obtained by dissolving CoCl_(3) in ammonia . The complex compound is denoted at [Co(NH)36-x]Cl_(3)-x (soluble 100% insible The chlorides shown inside the square breackets are not ionisable . The salt ioniss as [Co(NH_(3))_(6-x)Cl_(x)]Cl_(3-x)rarr[Co(NH_(3))_(6-x)Cl_(x)]^(+(3-x))+(3-x)Cl 0.1M CoCl_(3).xNH_(3) solution is found to boil t 100.104^(@)C (Kb "of water "=0.52K Kg "mol"^(-1)) What x? 'alpha' of salt =1)

A 0.001 molal solution of a complex represented as Pt(NH_(3))_(4)Cl_(4) in water had freezing point depression of 0.0054^(@)C . Given K_(f) for H_(2)O=1.86 K m^(-1) . Assuming 100% ionization of the complex, write the ionization nature and formula or complex.

A 0.001 molal solution of a complex represented as Pt(NH_(3))_(4)Cl_(4) in water had freezing point depression of 0.0054^(@)C . Given K_(f) for H_(2)O=1.86 K m^(-1) . Assuming 100% ionization of the complex, write the ionization nature and formula or complex.

A 0.001 molal solution of a complex represented as Pt(NH_(3))_(4)Cl_(4) in water had freezing point depression of 0.0054^(@)C . Given K_(f) for H_(2)O=1.86 K m^(-1) . Assuming 100% ionization of the complex, write the ionization nature and formula or complex.