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2.1 g of non-electrolyte solute (molar m...

2.1 g of non-electrolyte solute (molar mass 250 g/mol) was dissolved in 5.12 g of benzene. If the freezing point of depression constant, `k_f` of benzene is 5.12 K kg/mol, Calculate the freezing point of solution if freezing point of pure benzene is 5.5^0 C.

Answer

Step by step text solution for 2.1 g of non-electrolyte solute (molar mass 250 g/mol) was dissolved in 5.12 g of benzene. If the freezing point of depression constant, k_f of benzene is 5.12 K kg/mol, Calculate the freezing point of solution if freezing point of pure benzene is 5.5^0 C. by CHEMISTRY experts to help you in doubts & scoring excellent marks in Class 12 exams.

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Knowledge Check

  • 1 g of non - electrolyte solute (molar mass 250 g/mol) was dissolved in 5.12g of benzene. If the freezing point of depression constant, k_f of benzene is 5.12 K kg/mol, the freezing point of benzene will be lowered by

    A
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    B
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    C
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    D
    0.4 K
  • 31g of ethlylene glycol (C_2H_6O_2) is mixed with 500 g of solvent (K_f of the solvent is 2 K kg mol^-1) . What is the freezing point of the solution in K?

    A
    272
    B
    271
    C
    270
    D
    274
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