Solutions and Mixtures - AP Chemistry

1. What does $i$ represent in colligative property equations?

   $i$ is the van 't Hoff factor, representing ion count from a solute. Accounts for ionic dissociation in solution.

2. What is the definition of a solution?

   A homogeneous mixture of two or more substances. Components are uniformly distributed at molecular level.

3. What is the common ion effect?

   The suppression of solubility due to a common ion in solution. Shared ion reduces solubility of ionic compound.

4. Calculate the freezing point depression if $K_f = 1.86$, $m = 1$, and $i = 2$.

   $\triangle T_f = 3.72$ °C. Using $\triangle T_f = i \times K_f \times m = 2 \times 1.86 \times 1$.

5. What is the formula for mole fraction?

   Mole fraction = $\frac{\text{moles of component}}{\text{total moles of all components}}$. Dimensionless ratio expressing relative amounts.

6. What is the general effect of temperature on solid solubility?

   Solid solubility generally increases with temperature. More thermal energy overcomes lattice forces.

7. Calculate molality of a solution with 3 moles solute in 2 kg solvent.

   Molality = 1.5 mol/kg. Using $m = \frac{3 \text{ mol}}{2 \text{ kg}}$.

8. What is the common ion effect?

   The suppression of solubility due to a common ion in solution. Shared ion reduces solubility of ionic compound.

9. Calculate mass percent if 5g solute is in 95g solution.

   Mass percent = 5%. Using $\frac{5g}{100g} \times 100\%$.

10. What is the solute in a solution?

    The substance dissolved in the solvent. The minor component that gets dissolved.

11. What is the formula for mass percent?

    Mass percent = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 100$. Percentage concentration by mass composition.

12. Calculate the molarity of a solution with 2 moles of solute in 4 liters of solution.

    Molarity = 0.5 M. Using $M = \frac{2 \text{ mol}}{4 \text{ L}}$.

13. Define a supersaturated solution.

    A solution that contains more solute than it can theoretically hold at a given temperature. Unstable solution beyond normal solubility limit.

14. Calculate the mole fraction of solute in a solution with 1 mole solute and 3 moles solvent.

    Mole fraction = 0.25. Using $\frac{1}{1+3} = \frac{1}{4}$.

15. What does the symbol $X$ represent in Raoult's Law?

    $X$ represents the mole fraction of the solvent. Mole fraction shows proportion of solvent molecules.

16. What is an electrolyte solution?

    A solution that conducts electricity due to dissociated ions. Ions enable current flow through solution.

17. Define colligative properties.

    Properties that depend on the number of solute particles, not their identity. Particle count matters, not chemical identity.

18. What is the solute in a solution?

    The substance dissolved in the solvent. The minor component that gets dissolved.

19. State the formula for molarity.

    Molarity (M) = $\frac{\text{moles of solute}}{\text{liters of solution}}$. Concentration measured as moles per liter of solution.

20. Define the term 'immiscible'.

    Two liquids that do not mix to form a solution. Separate phases form due to different polarities.

21. What is the definition of a saturated solution?

    A solution in which no more solute can dissolve at a given temperature. Equilibrium reached between dissolving and crystallizing.

22. What is the relationship between particle size and rate of dissolution?

    Smaller particles dissolve faster due to larger surface area. Greater surface contact increases dissolution rate.

23. Calculate mass percent if 5g solute is in 95g solution.

    Mass percent = 5%. Using $\frac{5g}{100g} \times 100\%$.

24. Identify the definition of molality.

    Molality = $\frac{\text{moles of solute}}{\text{kilograms of solvent}}$. Concentration based on mass of solvent, not solution.

25. What is Henry's Law?

    The solubility of a gas is directly proportional to its pressure above the solution. Higher pressure forces more gas into solution.

26. What is the definition of a suspension?

    A heterogeneous mixture where particles settle out over time. Large particles visible and settle under gravity.

27. What is the solvent in a solution?

    The substance in which the solute is dissolved. The major component that does the dissolving.

28. What is an electrolyte solution?

    A solution that conducts electricity due to dissociated ions. Ions enable current flow through solution.

29. Calculate mass percent if 5g solute is in 95g solution.

    Mass percent = 5%. Using $\frac{5g}{100g} \times 100\%$.

30. What is the definition of solubility?

    The maximum amount of solute that can dissolve in a solvent at a given temperature. Temperature and pressure dependent dissolution limit.

31. What is the solvent in a solution?

    The substance in which the solute is dissolved. The major component that does the dissolving.

32. State the definition of a colloid.

    A mixture where dispersed particles do not settle out. Intermediate size between solutions and suspensions.

33. What is the solute in a solution?

    The substance dissolved in the solvent. The minor component that gets dissolved.

34. Define the term 'miscible'.

    Two liquids that are completely soluble in each other in all proportions. Complete mixing occurs at any ratio.

35. What is an unsaturated solution?

    A solution that can dissolve more solute at a given temperature. More solute can still be added and dissolved.

36. What is the effect of pressure on gas solubility?

    Gas solubility increases with increasing pressure. Follows Henry's Law for gas-liquid equilibrium.

37. What is Raoult's Law?

    $P_solution = X_solvent \times P^0_solvent$. Vapor pressure lowering due to solute presence.

38. Identify the process of solvation.

    The process of surrounding solute particles with solvent molecules. Solvent molecules form cage around solute.

39. Identify the relationship between temperature and gas solubility.

    Gas solubility decreases as temperature increases. Higher temperature reduces gas-liquid attractions.

40. What is the solvent in a solution?

    The substance in which the solute is dissolved. The major component that does the dissolving.

41. Identify the unit of molarity.

    Moles per liter (mol/L). Standard concentration unit for molarity calculations.

42. What is the unit of molality?

    Moles per kilogram (mol/kg). Temperature-independent concentration unit.

43. Define a non-electrolyte solution.

    A solution that does not conduct electricity. No ions present to carry electrical current.

44. What is the common ion effect?

    The suppression of solubility due to a common ion in solution. Shared ion reduces solubility of ionic compound.

45. Find the boiling point elevation if $K_b = 0.512$, $m = 2$, and $i = 1$.

    $\triangle T_b = 1.024$ °C. Using $\triangle T_b = i \times K_b \times m = 1 \times 0.512 \times 2$.

46. What is the Tyndall effect?

    The scattering of light by colloidal particles. Light beam becomes visible through colloid.

47. What is the formula for freezing point depression?

    $\triangle T_f = i \times K_f \times m$. Freezing point lowers with solute concentration.

48. What is an electrolyte solution?

    A solution that conducts electricity due to dissociated ions. Ions enable current flow through solution.

49. Identify the formula for boiling point elevation.

    $\triangle T_b = i \times K_b \times m$. Boiling point rises with solute concentration.

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