Home
Class 12
CHEMISTRY
A complex is represented as CoCl(3) . XN...

A complex is represented as `CoCl_(3) . XNH_(3)`. Its `0.1` molal solution in aqueous solution shows `Delta T_(f) = 0.558^(circ). (K_(f)` for `H_(2)O` is `1.86 K "molality"^(-1))` Assuming `100%` ionisation of complex and co-ordination number of `Co` as six, calculate formula of complex.

Text Solution

Verified by Experts

The correct Answer is:
`[Co(NH_(3))_(5)Cl]Cl_(2)`
Promotional Banner

Topper's Solved these Questions

  • LIQUID SOLUTION

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE) level-I|55 Videos

  • LIQUID SOLUTION

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE) level-II|30 Videos

  • LIQUID SOLUTION

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (SUBJECTIVE) level-I (NUMERICAL BASED PROBLEMS)|8 Videos

  • IONIC EQUILIBRIUM

    FIITJEE|Exercise SINGLE INTEGER ANSWER QUESTIONS|4 Videos

  • NUCLEIC ACID AND VITAMIN

    FIITJEE|Exercise ASSIGNMENT PROBLEMS (OBJECTIVE)|15 Videos

Similar Questions

Explore conceptually related problems

A complex is represented as CoCl_(3)Xnh_(3) . Its 0.1 molal solution in water DeltaT_(f)=0.588 K. K_(f) for H_(2)O is 1.86K" molality"^(-1) . Assuming 100% ionisation of complex and co - ordination number of Co is six calculate formula of 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.

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) for water is 1.86K kg mol^(-1) , the lowering in freezing point of the solution is

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

For [CrCl_(3).xNH_(3)] , elevation in b.pt of one molal solution is triple of one molal aqueous solution of urea. Assuming 100% ionisation of complex molecule, calculated the value of x .

An aqueous solution of urea has freezing point of -0.52^(@)C . If molarity and molality are same and K'_(f) for H_(2)O = 1.86 K "molality"^(-1) the osmotic pressure of solution would be:

Calculate the molecular weight of a substance whose 7.0% (by weight) solution in water freezes at -0.89^(@)C . (k_(f) "for" H_(2)O=1.86K"molality"^(-1) ).