Home
Class 12
CHEMISTRY
0.1M K(4)[Fe(CN)(6)] is 60% ionized. Wha...


0.1M `K_(4)[Fe(CN)_(6)]` is 60% ionized. What will be its van't Hoff factor ?

A

`1.4`

B

`2.4`

C

`3.4`

D

`4.4`

Text Solution

Verified by Experts

The correct Answer is:
C
`alpha= (i-1)/(n-1), n=5` since, `K_(4)[Fe(CN)_(6)]` gives 5 ions in the solution
`0.6 = (i-1)/(5-1)i=3.4`
Promotional Banner

Topper's Solved these Questions

  • SOLUTIONS

    BRILLIANT PUBLICATION|Exercise Level-III (Statement Type)|6 Videos

  • SOLID STATE

    BRILLIANT PUBLICATION|Exercise LEVEL-3 (Linked Comprehension Type)|10 Videos

  • STEREOCHEMISTRY

    BRILLIANT PUBLICATION|Exercise LEVEL-II (ASSERTION - REASON TYPE)|2 Videos

Similar Questions

Explore conceptually related problems

What is the significant of van't Hoff factor ?

If alpha=50%" for "K_(4) [Fe(CN)_(6)] , find out van't Hoff factor 'I'.

A 0.10 M aqueous solution of a monoprotic acid ("d=1.01 g/cm"^3) is 5% ionized. What is the freezing point of the solution? The mol.wt. of the acid is 300 and K_f (H_(2)O)="1.86"^@C//m:

The extend to which a solute is dissociated or associated can be expressed by Van't Hoff factor. Substantiate the statement.

The osmotic pressures of 0.010 M solutions of KI and of sucrose (C_(12)H_(22)O_(11)) are 0.432 atm and 0.24 atm respectively. The vant's Hoff factor for KI is:

The value of molecular mass determined by colligative properties are sometimes incorrect. What is Van't Hoff factor ?

The degree of dissociation (alpha) of a weak electrolyte, A_(x)B_(y), is related to van't Hoff factor (i) by the expression

In K_4[Fe(CN)_6] central metal Ion is ………..