Colligative Properties
Colligative properties, crucial in the study of solutions, are physical characteristics dependent solely on the number of solute particles, irrespective of their identity. These properties, including osmotic pressure, boiling point elevation, freezing point depression, and vapor pressure lowering, offer valuable insights into the behavior of solutions. As an essential concept in chemistry, colligative properties enable scientists to predict and manipulate the properties of solutions based on the concentration of solutes. Understanding these phenomena not only enhances practical applications in various industries but also contributes to the foundational knowledge of the interactions between solvents and solutes.
Questions
- When 3 grams of #"NaCl"# are added to 75.25 grams of water, what is the change in the water's freezing point?
- What is the boiling point of an aqueous solution of #"CaCl"_2# with a molal concentration of 1.56 mol/kg?
- Salt, NaCl, has a solubility of 35.7g per 100g of water at 0 degrees C. What is the lowest possible melting point for ice that could be obtained considering the solubility of NaCl in water? The Kf for H2O is 1.86 C/m
- What is the new boiling point for an aqueous #"0.743 molal"# solution of #"KCl"#? #K_b = 0.512^@ "C/m"#
- Consider two solutions: one formed by adding 10 g of glucose, C6H12O6, to 1 L of water and another formed by adding 10 g of sucrose, C12H22O11, to 1 L of water. Are the vapor pressures the same?
- What is the expected boiling-point elevation of water for a solution that contains 150 g of sodium chloride dissolved in 1.0 kg of water?
- How does the nature of the solute affect boiling point?
- How would you determine the vapor pressure of a solution at 25C that contains 76.6 g of glucose (C6H12O6) in 250.0 mL of water? The vapor pressure of pure water at 25C is 23.8 torr.
- Which of the given solutions should display the GREATEST departure from the freezing point, and the boiling point of the water solvent?
- Assuming 100% dissociation, what is the freezing point and boiling point of 3.39 m #K_3PO_4(aq)#?
- What is the freezing point of a nonionizing antifreeze solution containing 388g ethylene glycol #C_2H_6O_2# and 409 g of water?
- If #"14 g"# of calcium nitrate is dissolved in #"200 g"# of water, and it experiences a #70%# dissociation, what is the solution's vapor pressure if the solvent began at the normal boiling point of water? Hint: the normal boiling point occurs at 760 torr.
- What is the molar mass of the solute if #"4.18 g"# of it dissolved in #"36.30 g"# of benzene (#K_f = 5.12^@ "C"cdot"kg/mol"#) generates a solution with a freezing point of #2.70^@ "C"#? The freezing point of benzene is #5.53^@ "C"#.
- What is the boiling point of a solution made by dissolving 31 g of NaCl in 559 g of water?
- In making candy, a certain recipe calls for heating an aqueous sucrose solution to the "softball" stage. Which has a boiling point of 235-240 F. Wat is the range of mass percentages of the solution of sugar (C12H22O12) that boils at those two temperature?
- What do colligative properties depend on?
- What are three colligative properties of solutions?
- What is the molality of a solution of phosphoric acid, #H_3PO_4# that contains 24.5 g of phosphoric acid (molar mass 98.0 g) in 100 g of #H_2O#?
- A solution that contains #"13.2 g"# of solute in #"250 g"# of #"CCl"_4# freezes at #-33^@ "C"#. What is the FW of the solute? #T_f^"*"# of #"CCl"_4# is #-22.8^@ "C"# and its #K_f = -29.8^@ "C/m"#.
- What is the boiling point elevation formula?