Home
Class 12
CHEMISTRY
The osmotic pressure of 0.01 molar solut...

The osmotic pressure of 0.01 molar solution of an electrolyte is found to be 0.65 atm at `27^(@)C`. Calculate the van.t Hoff factor. What conclusion can you draw about the molecular state of the solute in the solution?

Text Solution

Verified by Experts

For electrolytes, `pi=i(n)/(V)RT`
where .i. is the vant Hoff factor
According to the given data, `pi = 0.65` atm
`R= 0.0821 " atm mol"^(-1)K^(-1)`
`T=27+273 =300K, n=0.01 "mol", V=1L`
Substituting the values, in the relation,
`pi= i(n)/(V)RT`, we get
`pi= 0.65 = (i xx 0.01)/(1) xx 0.0821L" atm mol"^(-1)K^(-1) xx 300 K`
`=0.246`i atm
`i=(0.65)/(0.246)=2.64`
Since `i gt 1`, the electrolyte undergoes dissociation.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • SOLUTIONS

    ICSE|Exercise MULTIPLE CHOICE QUESTIONS |23 Videos

  • SOLUTIONS

    ICSE|Exercise MULTIPLE CHOICE QUESTIONS (Fill in the blanks)|7 Videos

  • SOLUTIONS

    ICSE|Exercise ISC EXAMINATION QUESTIONS (PART-II Descriptive Questions) |11 Videos

  • SOLID STATE

    ICSE|Exercise ISC EXAMINATION QUESTIONS PART-I (Numerical Problems)|6 Videos

  • SOME IMPORTANT ORGANIC NAME REACTIONS

    ICSE|Exercise Questions |278 Videos

Similar Questions

Explore conceptually related problems

The osmotic pressure of 0.1 M sodium chloride solution at 27^@C is

The osmotic pressure of a solution containing 0.1 mol of solute per litre at 273 K is

Knowledge Check

  • The freezing point depression of 0.1 molal solution of acetic acid in benzene is 0.256 K , K_(f) for benzene is 5.12 K Kg mol^(-1) . What conclusion can you draw about the molecular state of acetic acid in benzence ?

    A
    Acetic acid is doubly associated
    B
    Benzene is doubly associated
    C
    Both are equally associated
    D
    None of the above.

    • Similar Questions

    Explore conceptually related problems

    The osmotic pressure of a solution containing 0.1 mol of solute per litre at 300 K is

    The osmotic pressure of a solution containing 0.1 mol of solute per litre at 323 K is

    The osmotic pressure of 0.1 M glucose and 0.1 M sucrose solution are the same because

    x g of non-electrolytic compound (molar mass =200) is dissolved in 1.0 L of 0.05 M NaCl solution. The osmotic pressure of this solution is found to be 4.92 atm at 27^(@)C . Calculate the value of x . Assume complete dissociation of NaCl and ideal behaviour of this solution.

    The osmotic pressures of 0.010 M solutions of KI and sucrose ( C_(12)H_(22)O_(11) ) are 0.432 atm and 0.24 atm respectively. The van't Hoff fector for KI is :

    The freezing point depression of 0.1 molal NaCl solution is 0.372 K. What conclusion can you draw about the molecular state of NaCl in water. K_f of water = 1.86 k/m.

    A 1.17% solution of NaCl is isotonic with 7.2% solution of glucose. Calculate the Van't Hoff factor of NaCl .

    Home
    Profile