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Solutions Review

Solutions Review. How much of the solute will dissolve and how much will remain undissolved at the bottom of the test tube? 60g of N aCl in 100g of water at 60ºc. 40g dissolved 20 g undissolved.

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Solutions Review

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  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

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