What mass of ethlene ethyelne glycol `("molar mass"=62 g mol^(-1))` must be dissolved in 5.5kg of water to lower the freezing point of from `0^(@)C to-10^(@)C` ? `(K_(f))` for water=1.86 K kg `mol^(-1)`).

What mass of ethylene glycol (molar mass = "62.0 g mol"^(-1) ) must be added to 5.50 kg of water to lower the freezing point of water from 0^(@)C to -10.0^(@)C ( k_(f) for water = "1.86 K kg mol"^(-1) ).

What mass of ethylene glycol (molar mass = 62.0 g mol^(-1) ) must be added to 5.50 kg of water to lower the freezing point of water from 0^(@)C to - 10.0^(@) C ? (K_(f) "for water " = 1.86 k " kg mol"^(-1))

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.

What mass of NaCl (molar mass= 58.5g mol^-1) must be dissolved in 65g of water to lower the freezing point by 7.5^@C ? The freezing point depression constant, K_f for water is 1.86 K kg mol^-1 . Assume vant Hoff factor for NaCl is 1.87.

What mass of NaCl ("molar mass =58.5 g mol"^(-1)) dissolved in 50g of water will lower the freezing point by 5^@C? The freezing point depression constant, K_p for water is 1.86" K kg mol"^(-1) , van't Hoff factor for NaCl is 1.87.

How many grams of ethylene glycol (molar mass = 62) should be added to 10 kg of water, so that the resulting solution freezes at -10^(@)C ( K_(f) for water = 1.86 K "mol^(-1) ).

Calculate the mass of compound (molar mass = 256 g mol^(-1) ) to be dissolved in 75 g of benzene to lower its freezing point by 0.48 K(K_(f) = 5.12 " K kg " mol^(-1)) .