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Comprehensive Review of Solution Chemistry Concepts

This review covers essential concepts in solution chemistry, including saturation levels, molarity calculations, and the effects of temperature on solubility. You'll explore how to prepare specific molar solutions, determine molarity from mass and volume, and understand the principles governing dissolving processes. Key questions include the impact of heating on solubility, the precipitation of solutes when solutions are cooled, and the conditions that affect gas solubility. Additionally, the review addresses the nature of electrolytes and the significance of ionization and solubility principles.

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Comprehensive Review of Solution Chemistry Concepts

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  1. Unit 10 Review *For Bonus

  2. # 1. (3) A solution that contains the maximum amount solute per solvent at a given temperature is said to be ____________________.

  3. # 2 (4) You have a solution that is 1.5M H2SO4. How many mL of this acid do you need to prepare 100.0 mL of 0.18M H2SO4?

  4. #3 (4) A 0.0678 g sample of NaCl is dissolved in 100 mL of water. What is the molarity of this solution?

  5. #4 (3) What do the lines in the graph represent?

  6. #5 (3) Does heating a solution increase or decrease the solubility of a solid?

  7. #6 (4) A saturated solution of NaNO3 at 50oC is cooled to 20oC. Approximately how much solute will precipitate out of solution?

  8. #7 (3) What are the 3 conditions required to get a gas to dissolve better/faster in a solution?

  9. # 8 (5) 50 g of KClO3 are added to 100g of water at 40oC. Approximately how much solute is left undissolved at the bottom of the container?

  10. #9 (3) What are the 3 conditions in which a solid will dissolve better or faster in solution?

  11. #10 (3) What is an electrolyte?

  12. #11 (5) What volume of solution is required to produce a 2 M solution that contains 0.28 moles of solute?

  13. #12 (3) What does it mean when a salt ionizes in solution?

  14. #13 (4) How many grams of KNO3 are required to make a saturated solution at 60oC?

  15. #14 (3) What does the phrase “like dissolves like” referring to?

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