Solutions Review

1. Solutions Review

2. How much of the solute will dissolve and how much will remain undissolved at the bottom of the test tube?60g of NaCl in 100g of water at 60ºc • 40g dissolved • 20 g undissolved

3. Suppose you were making a salt water solution. Sodium ions and chloride ions are separating from one another. What is this called? • Dissociation

4. What are the 3 different types of mixtures? • Solutions • Suspensions • Colloids

5. Describe how stirring increases the rate of dissolving of a solute. • Allows continual contact between solute & solvent

6. What type of mixture are colloids classified as? • Heterogeneous

7. ___________ is a homogeneous mixture • Solutions

8. What is an example of a colloid? • Aerosols • Foams • Emulsions • Gels/Sols

9. Explain why a beaker of NaCl crystals cannot conduct an electrical current. Be specific. • Ions are not dissociated and the ions are not mobile since the are not in a solution

10. ________ is the substance that does the dissolving in a solution • Solvent

11. _______ is a substance that dissolves in water to give a solution that conducts electric current • Electrolyte

12. What are the 3 factors that can increase the solution rate? • Heating • Stirring • Grinding

13. Describe how heating increases the rate of dissolving of a solute. • Increases the kinetic energy so molecules are moving faster so more collisions between the solute & solvent

14. Determine what type of mixture a substance is by the following observation : particles are scattered by light • Colloid

15. At 100°C, 70g of NaCl is dissolved in 100g of water. Is this solution saturated or unsaturated? • Saturated

16. What is solution equilibrium? • State where the solute is dissolving at the same rate that the solute is coming out of solution (crystallizing).

17. _____ is the quantity of solute that will dissolve in specific amount of solvent at a certain temperature. • Solubility

18. Describe how grinding a solute increases the rate of dissolving. • Creates more of a surface area on the solute, so more collisions between solute & solvent will occur

19. Suppose you were making a salt water solution. Sodium ions and chloride ions are each being surrounded by water molecules. What is this called? • Solvation

20. _____ is a stable solution in which the maximum amount of solute has been dissolved • Saturated Solution

21. What helps to prevent colloid particles from settling out of a mixture? • Brownian Motion

22. Explain why a beaker of NaClwater can conduct an electrical current. Be specific. • Ions are dissociated and the ions are mobile

23. Determine what type of mixture A substance is by the following observation : particles can be separated by filtration • Suspension

24. _____ is the visible pattern caused by the reflection of light from suspended particles in a colloid • Tyndall Effect

25. What is visual evidence that a solution would be saturated? • Undissolved solute would be present at the bottom of the container

26. _____ is the substance that gets dissolved in a solution • Solute

27. ____ is a solution that contains less solute than a saturated solution under existing conditions • Unsaturated

28. ____ is a mixture that is uniform in composition • Homogeneous

29. At 100°C, 10g of NaCl is dissolved in 100g of water. Is this solution saturated or unsaturated? • Unsaturated

30. What is considered the “universal solvent”? • water

31. What are 3 factors that affect solubility? • Nature of solutes/solvents • Temperature • Pressure

32. How many grams of potassium bromide can be dissolved in 100g of water at 80°C? • 98g

33. Explain the rule, “Like Dissolves Like”. • rule of thumb for predicting whether or not one substance dissolves in another • Ex: Polar solutes will dissolve in polar solvents

34. ____ is a colloid where solids and liquids dispersed in gases (fog) • Aerosols

35. Describe the 3 steps in the dissolving process. • Solute-solute attraction is broken up; requires energy • Solvent-solvent attraction is broken up; requires energy • Solute-solvent attraction is formed; releases enerty

36. _____ is a mixture in which the particles are so large that they settle out unless the mixture is constantly stirred or agitated • suspension

37. What is an example of a suspension? • Oil and water • Dirt and water

38. _____ is a mixture consisting of particles that are intermediate in size between those in solutions and those in suspensions • Colloid

39. What type of mixture are suspensions classified as? • Heterogeneous

40. ____is the random continuous motions of colloidal particles • Brownian Motion

41. _______ is a substance that dissolves in water to give a solution that DOES NOT conduct electric current • Nonelectrolyte

42. What is an example of the tyndall effect? • Visibility of headbeams on a foggy night

43. Which salt is least soluble at 60 °C? • NaCl

44. _____ is a solution that temporarily contains more than the saturation amount of solute than the solvent can hold (unstable) • Supersaturated

45. Which salt is MOST soluble at 20 °C? • NaClO3

46. What is an example of a solution? • Food coloring and water

47. ____ is a colloid where gases dispersed in liquids (Ex: whipped cream) • Foam

48. _____ is the separation of ions from each other in a solution • Dissociation

49. What is the molarity formula? (besides M1V1 = M2V2) • Molarity = Moles of Solute Liters of Solution

50. Explain why a sugar solution cannot conduct an electrical current. Be specific. • No charged particles are present and they are not mobile