13.9 The figure shows two identical volumetric flasks containing the same solution at two temperatures (a) Does the molarity of the solution change with the change in temperature? (b) Does the molality of the solution change with the change in temperature? [Section 13.4] 0at 55 °C 25 °C

An aqueous solution contains the amino acid glycine (NH2CH2COOH). Assuming that the acid does not ionize in water, calculate the molality, in molal, of the solution if it freezes at - 2.83 °C. (Cryoscopic constant of water: 1.86 °C/molal; Atomic Weight: N = 14.01 g/mol; H = 1.008 g/mol; C = 12.01 g/mol; O = 16.00 g/mol; density of water = 1.00 g/mL). Express your answer in three %3D decimal places only. Do not put the units.

Pentane (C3H12) and hexane (C,H14) form ideal solution. At 25°C the vapor pressure of pentane and hexane are 511 torr and 150. torr, respectively. A solution is prepared by mixing 30.0 mL pentane (density = 0.63 g/mL) with 45.0 mL hexane (density = 0.66 g/mL). (a) What are the mole fractions of pentane and hexane, respectively, in the solution? (b) What is the total vapor pressure of the solution at 25°C? (c) What are the mole percent of pentane and hexane, respectively, in the vapor phase at 25°C? (Molar mass of pentane and hexane are: 72.15 g/mol and 86.17 g/mol, respectively.)

acid, CH3COOH, is 1.0187 g/mL. What is (a) the molarity? (b) the molality? (c) the mole fraction of each component?