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What mass of NaCl (molar mass=58.5 g mol...

What mass of NaCl (molar mass=`58.5 g mol^-1`) must be dissolved in 65.0 g of water to lower the freezing point by `7.50 ^@C`? The freezing point depression constant, `K_f`, for water is `1.86 K kg mol^-1`. Assume Van's Hoff factor for NaCl is 1.87.

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What mass of NaCl must be dissolved in 65.0 g of water to lower the freezing point of water by 7.50^@C ? The freezing point depression constant (k_f) for water is 1.86^@C/m . Assume that Van't Hoff factor for NaCl is 1.87. (Molar mass of NaCl =58.5g).

Caculate the mass of a compound (molar mass=256g mol^-1) to be dissolved in 75g of benzene to lower its freezing point by 0.48K (K_f=5.12 K kg mol^-1)

1.00g of a non-electrolyte solute dissolved in 50g of benzene lowered the freezing point of benzene by 0.40K. The freezing point depression constant of benzene is 5.12K mol^-1 . Find the molar mass of the solute.

Calculate the amount of CaCl_(2) (molar mass = 111g "mol"^(-1) ) which must be added to 500 g of water of lower its freezing point by 2K, assuming CaCl_(2) is completely dissociated. (Kf for water = 1.86 k kg "mol"^(-1) ).

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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 benzene.

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MODERN PUBLICATION-SOLUTIONS -EXERCISE
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