G A certain liquid.I has a normal boiling point of 102.60 °C and a boiling point elevation constant K₂ = 0.85 °C-kg-mol¹. A solution is prepared by dissolving some ammonium sulfate ((NH4)2SO4) in 400. g of X. This solution boils at 103.8 °C. Calculate the mass of (NH4)2SO4 that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. g ☐ x10

The normal boiling point of a certain liquid X is 140.50 °C, but when 32.3 g of alanine (C,H,NO,) are dissolved in 250. g of X the solution boils at 141.7 °C instead. Use this information to calculate the molal boiling point elevation constant K, of Х. Round your answer to 2 significant digits. olo °C·kg Ar K, = [] mol

The freezing point of benzene, C6H₁, is 5.50 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in benzene is DDT. A student dissolves 11.78 grams of DDT, C14H9 C15 (354.5 g/mol), in 252.1 grams of benzene. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH3 CH₂ OH CHC13 C6H6 Diethyl ether CH3 CH₂ OCH2 CH3 The molality of the solution is The freezing point of the solution is Kb (°C/m) Kf (°C/m) 1.86 1.99 0.512 1.22 3.67 2.53 2.02 m. °C. 5.12

The molal boiling point elevation constant K,=0.90 °C·kg mol 1 for a certain substance X. When 26. g of urea ((NH.),CO) CO are dissolved in 650. g of X, the solution boils at 137.9 °C. Calculate the boiling point of pure X. Be sure your answer has the correct number of significant digits. °C x10

A 83.5 g sample of a nonelectrolyte is dissolved in 250.1 g of water. The solution is determined to have a boiling point of 102.3 °C. What is the molar mass of the compound? (Kb for water is 0.510 °C/m).

A solution is made by dissolving 38.750 g of sample of an unknown, nonelectrolyte compound in water. The mass of the solution is exactly 500.0 g. The boiling point of this solution is 100.220∘C. What is the molecular weight of the unknown compound?

At a certain temperature the vapor pressure of pure water is measured to be 233. mmHg. Suppose a solution is prepared by mixing 131. g of water and 71.8 g of acetic acid (HCH,CO2). Calculate the partial pressure of water vapor above this solution. Round your answer to 3 significant digits. Note for advanced students: you may assume the solution is ideal. | mmHg x10

The normal freezing point of a certain liquid X is 5.20 °C, but when 41. g of urea (CH,N,O) are dissolved in 750. g of X the solution freezes at 2.5 °C instead. Use this information to calculate the molal freezing point depression constant K, of Х. Round your answer to 2 significant digits. °C·kg x10 K, = 0 mol

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