Home
Class 12
CHEMISTRY
Show graphically that the freezing point...

Show graphically that the freezing point of a liquid will be depressed when a non-volatile solute is dissolved in it. The freezing point of a solution containing 0-3 g of acetic acid in 30-0 g of benzene is lowered by 0-`45^@`. Calculate the van't Hoff factor. (K for benzene = 5-12 K kg mol`""^(-1)`).

Text Solution

Verified by Experts

Graphical representation of freezing point depression is given in Fig.
. Freezing point depression,
`Delta T_f =T_(f_f^(@) -T_f`
Let us first calculate observed molar mass.
`M_B=(K_fxxW_Bxx1000 )/( Delta T_f xx W_A)`
`=(5.12 xx 0.3 xx 1000)/(=5.12 xx 0.3 xx 1000)/(0.45 xx 30.0 )`
`113.8`

Normal molar mass of CH3COOH = 60
Van.t Hoff factor, i = `("Normal molar mass")/("Observed molar mass ")`
`=(60)/(113.8)= 0.527`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • SOLUTIONS

    MBD -HARYANA BOARD|Exercise SATQ (SHORT ANSWERS TYPE QUESTIONS )|16 Videos

  • SOLID STATE

    MBD -HARYANA BOARD|Exercise LONG ANSWER TYPE QUESTIONS|10 Videos

  • SURFACE CHEMISTRY

    MBD -HARYANA BOARD|Exercise LONG ANSWER TYPE QUESTIONS|4 Videos

Similar Questions

Explore conceptually related problems

The freezing point of a solution contaning 0.3 g of acetic acid in 43 g of benzene reduces by 0.3^(@) . Calculate the Van's Hoff factor "( K_(f) for benzene = 5.12 K kg mol^(-1) )"

The freezing point of a solution containing 0.3 g of acetic acid in 30 g of acetic acid in 30 g of benzene is lowerd by 0.54^(@) , Calculate Van't Hoff factor. (K_(f)" for benzene"= 5.12 " K kg mol"^(-1) ).

Knowledge Check

  • The freezing point of a solution containing 0.2 g of acetic acid in 20.0 g benzene is lowered by 0.45^@C . The degree of association of acetic acid in benzene is (Assume acetic acid dimerises in benzene and K_f for benzene = 5.12 K kg "mol"^(-1) ) ?

    A
    `94.6%`
    B
    `54.9%`
    C
    `78.2%`
    D
    `100%`

    • Similar Questions

    Explore conceptually related problems

    The freezing point of a solution containing 0.2 g of acetic acid in 20.0 g of benzene is lowered by 0.45^@C . Calculate the degree of association of acetic acid in benzene. K_f(C_6H_6) = 5.12 K "mol"^(-1) kg

    The freezing point of solution containing 0.2 g of acetic acid in 20.0 g of benzene is lowered by 0.45^(@)C . Calculate the degree of association of acetic acid in benzene. (K_(f)=5.12 K^(@) mol^(-1) kg^(-1))

    Phenol associates in benzene to a certain extent to form a dimmer. A solution containing 20 g of phenol in 1.0 kg of benzene has its freezing point lowered by 0.69 K. Calculate the fraction of phenol that has dimerised. [Given K_f for benzene = 5.1 K m^(-1)

    0.15 molal solution of NaCI has freezing point -0.52 ^(@)C Calculate van't Hoff factor . (K_(f) = 1.86 K kg mol^(-1) )

    Calculate the molecular weight of a substance if the freezing point of a solution containing 100 g of benzene and 0.2 g of the substance is 0.17 K below that of benzene. The cryoscope constant of benzerne is 5.16 K kgmol^(-1)

    The freezing point depression constant of benzene is 5.12 K kg mol^(-1) . The freezing point depression for the solution of molality 0.078m containing a non-electrolyte solute in benzene is

    The freezing point of benzene decreases by 2.12 K when 2.5 g of benzoic acid (C_6H_3COOH) is dissolved in 25 g of benzene. If benzoic acid forms a dimer in benzene, calculate the van't Hoff factor and the percentage association of benzoic acid. [ K_f for benzene = 5.12 K kg "mol"^(-1) ]

    Home
    Profile