An aqueous solution contains the amino acid glycine (NH2CH2COOH). Assuming that the acid does not ionize in water, calculate the molality of the solution if it freezes at -1.67°C. Be sure your answer has the correct number of significant digits. Note: Reference the Molal freezing point depression and boiling point elevation constants table for additional information. m x x10 ×

1 for a certain substance X. When 38.6 g of urea (NH,), CO) The molal boiling point elevation constant K, =1.54 °C·kg mol are dissolved in 950. g of X, the 9. 2 solution boils at 113.3 °C. Calculate the boiling point of pure X. Round your answer to 4 significant digits. x10

A certain liquid X has a normal freezing point of 0.90°C and a freezing point depression constant Kf=6.96·°C·kgmol−1.A solution is prepared by dissolving some barium hydroxide (Ba(OH)2) in 900.g of X. This solution freezes at−3.7°C. Calculate the mass of Ba(OH)2 that was dissolved. Round your answer to 2 significant digits.

The normal boiling point of a certain liquid X is 141.80 °C, but when 60.9 g of iron(III) nitrate (Fe(NO3)) are dissolved in 400. g of X the solution boils at 142.8 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. olo °C·kg K, = ] Ar х10 mol

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

The molal boiling point elevation constant K = 1.15 °C·kg⋅mol the solution boils at 145.4 °C. Calculate the boiling point of pure X. Be sure your answer has the correct number of significant digits. °C x10 1 for a certain substance X. When 14.4 g of urea Ś ((NH,),CO) (NH₂) CO) are dissolved in 150. g of X,

A certain liquid X has a normal boiling point of 92.90°C and a boiling point elevation constant Kb=2.15·°C·kgmol−1. Calculate the boiling point of a solution made of 30.g of potassium bromide (KBr) dissolved in 800.g of X. Round your answer to 3 significant digits.

1 A certain liquid X has a normal freezing point of 0.40 °C and a freezing point depression constant K = 5.78 °C·kg⋅mol A solution is prepared by dissolving some glycine (C₂HÃNO₂) in 850. g of X. This solution freezes at −5.2 °C. Calculate the mass of C₂H²NO₂ that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. 1 g | x10 S

When 911. mg of a certain molecular compound X are dissolved in 35.0 g of benzene (C,H6), the freezing point of the solution is measured to be 2.5 °C. Calculate the molar mass of X. If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. Ox10 미□

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