A certain liquid X has a normal freezing point of -3.00 °C and a freezing point depression constant K, 4.23 °C-kg-mol. Calculate the freezing point of a solution made of 72.3g of ammonium sulfate ((NH4), SO4) dissolved in 750. g of X. Round you answer to 4 significant digits. °C X S

Ethylene glycol (C₂H₆O₂) is used as an additive to the water in your automobile to lower its freezing point. A solution of ethylene glycol in water has a freezing point of -8.80°C. What is the mole fraction of ethylene glycol in this solution? (Kf for water is 1.86°C･kg/mol). Please use the correct significant figures. Thank you!

A solution of 4.63 g of anhydrous aluminum chloride (AlCl3) in 59.08 g of water freezes at -4.37 degrees celsius. Kf (AlCl3) =1.86 degrees celsius/m part 1: calculate the molar mass of AlCl3 from the formula. Round the answer to the hundredths place. ___ g/mol Part 2: Calculate the molar mass from the freezing point depression, assuming AlCl3 does not dissociate in ions. Round to 3 Significant digits. Part 3: Comparing the two values, how many ions will AlCl3 form? Round the answer to the nearest whole number.

A solution was prepared by dissovling 0.800 g of sulfur, S8, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution. Boiling point 118.5 degrees C. Freezing point 16.60 degrees C. Kb = 3.08 degrees C/m. Kf = 3.59 degrees C/m.

Urea (NH2)2CO, is dissolved in 105.0 g of water. The solution freezes at -0.605°C. How many grams of urea were dissolved to make this solution? The Kf=1.858°C/m for water and its freezing point is 0.000°C. Express your answer to two decimal places.

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A certain liquid X has a normal freezing point of -9.00 °C and a freezing point depression constant K, = 7.04 °C-kg mol . A solution is prepared by dissolving some potassium bromide (KBr) in 400. g of X. This solution freezes at -13.6 °C. Calculate the mass of KBr that was dissolved. Round your answer to 2 significant digits.

The freezing point of water is 0.00 °C at 1 atmosphere. How many grams of cobalt(II) acetate (177.0 g/mol), must be dissolved in 245.0 grams of water to reduce the freezing point by 0.300 °C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Mass Water H₂O Ethanol CH3 CH₂OH 1.22 Chloroform CHC13 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 Kb (°C/m) Kf(°C/m) 0.512 g 1.86 1.99 5.12

What is the osmotic pressure in torr of a O.0173 M glucose solution at body temperature (37 °C)? What are the boiling and freezing points for the same solution? The osmotic pressure = i torr T= i °C Tbp= °C i [For this part, write your answer to the nearest ten-thousandth, rather than using significant figures rules.] P A O S MacBook Air

Solvent Formula Diethyl ether Water Ethanol Chloroform CHCl3 Benzene C6H6 H₂O CH3 CH₂ OH Kb (°C/m) K(°C/m) 0.512 The molality of the solution is The freezing point of the solution is 1.22 3.67 2.53 CH3 CH₂ OCH₂ CH3 2.02 m. 1.86 1.99 5.12 °C.