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Solution Chemistry Test Review Work Stations

Solution Chemistry Test Review Work Stations. Station 1 – Solubility Concepts. Identify the three factors that affect the rate of solution formation. Identify the two components of a solution. What units do we use to express solubility? What are the factors that affect solubility?

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Solution Chemistry Test Review Work Stations

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  1. Solution Chemistry Test Review Work Stations

  2. Station 1 – Solubility Concepts • Identify the three factors that affect the rate of solution formation. • Identify the two components of a solution. • What units do we use to express solubility? • What are the factors that affect solubility? • What does a solution look like when it is supersaturated? • How can you determine the saturation point of a substance using lab techniques? (HINT: think about the procedures of the “Solubility Curve Lab” from last week)

  3. Station 1 – Solubility Concepts Answer Key • 1. Agitation, temperature change, particle size • 2. Solute, solvent • 3. grams solute/100 g of solvent • 4. temperature and pressure • 5. solid precipitates out when cooled • 6. raise the solution until all solute dissolves. Lower temperature and record temperature at the instant solid crystals form in solution.

  4. Station 2 – Solubility Curves • See next slide for worksheet.

  5. Solubility WS DIRECTIONS: Use the solubility curve from the previous packet to answer the following questions. ___________1) What is the solubility of potassium nitrate in 100 grams of water at 20 °C ?___________2) What is the solubility of potassium chloride in 100 grams of water at 50 °C ?___________3 )What is the solubility of sodium chloride in 100 grams of water at 90 °C ? ___________4) What is the minimum temperature needed to dissolve 60 grams of potassium nitrate in 100 grams of water___________5) What is the minimum temperature needed to dissolve 35 grams of potassium chloride in 100 grams of water___________6) At what temperature do potassium chloride and potassium nitrate have the same solubility ?___________7) If 110 grams of potassium chloride are mixed with 100 grams of water at 20 °C, how much will not dissolve ?___________8) If 120 grams of potassium nitrate are mixed with 100 grams of water at 60 °C, how much will not dissolve ?___________9) If 15 grams of potassium chloride are added to 100 grams of water at 30 °C, how much more must be added to saturate the solution?___________10) If 85 grams of potassium nitrate are added to 100 grams of water at 70 °C, how much more must be added to saturate the solution?___________11) 100 grams of water at 95 °C are saturated with sodium chloride. If this solution is cooled to 35°C, how much of the solid will precipitate? ___________12) 100 grams of water at 90 °C are saturated with potassium chloride. If this solution is cooled to 35°C, how much of the solid will precipitate?___________13) How much potassium chlorate will dissolve in 200 grams of water at 70 °C ? ___________14) How much potassium nitrate will dissolve in 300 grams of water at 10 °C ? ___________15) How much potassium chloride will dissolve in 50 grams of water at 50 °C ?

  6. Station 2 – Solubility Curves • 34 g • 43 g • 39g • 37 °C • 25 °C • 20 °C • 76-77g • 7 g • 22g • 51-55 g • 2 g • 18 g • 70 g • 66 g • 21-22 g

  7. Station 3 – Molarity • 1. Define Molarity, then calculate the molarity of each solution: • 1.0 mol KCl in 750 mL of solution • 0.5 mol MgCl2 in 1.5 L of solution • 2. Calculate the moles and grams of solute in each solution: • 1.0L of 0.50 M NaCl • 500 mL of 2.0 M KNO3 • 250 mL of 0.10M CaCl2

  8. Station 3 – Molarity • 1. a.1.3 M KCl, b.0.33 M MgCl2 • 2. a. 0.5 mol NaCl, 29 g NaCl • b. 1.0 mol KNO3, 100 g KNO3 • C. 0.025 mol CaCl2, 2.8 g CaCl2

  9. Station 4- molality • 1. Distinguish between a 1 M solution and a 1 m solution. • Describe how you would prepare a 1.00 m solution of glucose. (i.e., grams of glucose needed in 1000 g of water?) • Describe how you would prepare a 0.500 m solution of sodium chloride. (i.e., grams of sodium chloride in 1000 g of water?)

  10. Station 4- molality • 1. 1 M solution: 1 mol of solute in 1 L of solution; 1 m solution: 1 mol of solute in 1000g/1 kg of solvent • 2. Dissolve 180 g (1 mole) of glucose in 1 kg of water. • 3. Dissolve 29.3 g of NaCl (0.5 mole) in 1 kg of water.

  11. Station 5 – Percent Solutions • 1. Calculate the grams of solute required to make the following solutions: • 2500 g of saline solution (0.90% NaCl (m/m)) • 0.050 kg of 4.0% (m/m) MgCl2 • What is the concentration ( in % (v/v)) of the following solutions? a) 25 mL of ethanol (C2H5OH) is diluted to a volume of 150 mL with water. • 175 mL of isopropyl alcohol (C3H7OH) is diluted with water to a total volume of 275 mL

  12. Station 5 – Percent Solutions • 1. a. 23 g NaCl B. 2.0 g MgCl2 • a. 16% (v/v) ethanol b. 63.6 % (v/v) isopropyl alcohol

  13. Station 6 – Molarity by Dilution • How many mL of 4.00 M KI are needed to prepare 250.0 mL of 0.760 M KI? • How could you prepare 250 mL of 0.20 M NaCl using only a solution of 1.0 M NaCl and water? • How many milliliters of 0.500 M KCl solution would you need to dilute to make 100.0 mL of 0.100 M KCl?

  14. Station 6 – Molarity by Dilution • 1. 47.5 mL • 2. Add 50 mL of the 1.0 M solution to a 250 mL volumetric flask, then fill to the mark. • 3. 20 mL.

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