Composition of Mixtures - AP Chemistry

1. What term is used for the maximum amount of solute that can dissolve in a solvent at a given temperature?

   Saturated solution. Equilibrium state where no more solute can dissolve.

2. Identify the property that describes how much solute can dissolve in a solvent at a given temperature.

   Solubility. Maximum amount of solute that dissolves at equilibrium conditions.

3. Identify the principal distinction between a homogeneous and a heterogeneous mixture.

   Homogeneous mixtures have uniform composition; heterogeneous do not. Homogeneous means uniform throughout; heterogeneous has visible distinct phases.

4. What is the formula for calculating the mole fraction of a component in a mixture?

   Mole fraction = $\frac{\text{moles of component}}{\text{total moles of all components}}$. Expresses relative amount of each component in molar terms.

5. Identify the effect of a solute on the freezing point of a solvent.

   Freezing point depression. Solute particles lower the freezing point below pure solvent.

6. What is the term for the layer that forms in a heterogeneous mixture of immiscible liquids?

   Interface. Boundary between two immiscible liquid phases in mixture.

7. What is the concentration unit defined as moles of solute per liter of solution?

   Molarity (M). Most common concentration unit for solutions in chemistry calculations.

8. Which term describes a mixture where particles are dispersed throughout but not dissolved?

   Colloid. Intermediate between solution and suspension with dispersed particles.

9. What effect does the addition of a solute have on the vapor pressure of a solvent?

   Vapor pressure reduction. Solute particles decrease vapor pressure below pure solvent value.

10. What is the usual effect of pressure on the solubility of solids in liquids?

    Little to no effect. Solid solubility typically independent of pressure changes.

11. Which type of mixture displays the Tyndall effect?

    Colloid. Light scattering distinguishes colloids from true solutions.

12. What is the effect of increasing temperature on the solubility of gases in liquids?

    Solubility of gases decreases with increasing temperature. Higher temperature reduces gas-liquid attractive forces and solubility.

13. Which rule determines the solubility of ionic compounds in water?

    Solubility rules. Empirical guidelines that predict which ionic compounds dissolve in water.

14. What does the term 'miscible' mean when describing two liquids?

    Liquids that are soluble in each other in all proportions. Complete solubility in each other at any ratio or proportion.

15. How do you express parts per million (ppm) in terms of mass?

    ppm = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 10^6$. Expresses very small concentrations as parts per million by mass ratio.

16. Which law relates the solubility of a gas in a liquid to the pressure of the gas above the liquid?

    Henry's Law. Gas solubility is directly proportional to partial pressure above liquid.

17. What is the term for the concentration of a solution expressed in equivalents per liter?

    Normality (N). Concentration based on chemical equivalents rather than moles.

18. What term describes a mixture that scatters light, known as the Tyndall effect?

    Colloid. Dispersed particles scatter light beams making them visible.

19. What is the formula for parts per billion (ppb) in terms of mass?

    ppb = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 10^9$. Even smaller concentrations expressed as parts per billion by mass.

20. What is the key feature of a suspension compared to a solution?

    Particles in a suspension are larger and settle over time. Large particles settle due to gravity, unlike dissolved solutions.

21. What defines a solution with equal concentrations of solute and solvent on either side of a membrane?

    Isotonic solution. Equal solute concentrations prevent net water movement across membrane.

22. What is the result of adding a non-volatile solute to a solvent in terms of boiling point?

    Boiling point elevation. Solute particles increase the boiling point above pure solvent.

23. What is the term for the pressure that must be applied to prevent osmotic movement across a selectively permeable membrane?

    Osmotic pressure. Pressure needed to stop solvent flow across semipermeable membrane.

24. What is the key distinction between a colloid and a true solution?

    Colloids have larger particles than true solutions. Colloid particles are larger but still small enough to remain dispersed.

25. Which process involves the separation of a mixture by passing it through a medium where components move at different rates?

    Chromatography. Components move through medium at different rates enabling separation.

26. What is the formula for molality of a solution?

    Molality = $\frac{\text{moles of solute}}{\text{kilograms of solvent}}$. Temperature-independent concentration based on solvent mass, not volume.

27. Which separation method involves heating a liquid to create vapor and then cooling the vapor to get liquid?

    Distillation. Vaporization followed by condensation separates by volatility differences.

28. Which term denotes the concentration of a solution in terms of mole fraction?

    Mole fraction. Ratio of component moles to total moles in mixture.

29. What is the term for a solution with a pH greater than 7?

    Basic (or alkaline) solution. Low hydrogen ion concentration creates basic conditions.

30. What is the formula for calculating the dilution of a solution?

    $M_1V_1 = M_2V_2$. Conservation relationship for diluting concentrated solutions to lower concentrations.

31. What is a common method for separating a solid from a liquid in a heterogeneous mixture?

    Filtration. Physical separation using porous barrier to retain solid particles.

32. What is the formula for calculating the mass percent of a component in a mixture?

    Mass percent = $\frac{\text{mass of component}}{\text{total mass of mixture}} \times 100$. Standard formula expressing component mass as percentage of total mixture mass.

33. What is the term for a solution that has a pH less than 7?

    Acidic solution. High hydrogen ion concentration creates acidic conditions.

34. What is the technique called that separates mixtures based on differences in density?

    Centrifugation. High-speed spinning separates components by density differences.

35. What term describes a solution that contains more solute than it can theoretically hold at a given temperature?

    Supersaturated solution. Unstable solution exceeding normal solubility limit at that temperature.

36. What term describes the component of a solution present in the greatest amount?

    Solvent. The major component that dissolves other substances in a solution.

37. Which technique uses a semi-permeable membrane to separate small particles from large ones?

    Dialysis. Membrane separation based on particle size differences.

38. What is the term for the process of separating a mixture into its components based on boiling points?

    Distillation. Separation technique exploiting different boiling points of components.

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