Independent Practice 1 Name: Unit 2: Solutions Class Period: Final Due Date: Quiz Date: Learning Target A: Components of a Solution 1. In the illustration below, label and define the following terms: solute, solvent, solution. 2. Read the following passage regarding solubility and answer the questions that follow. What do you think would happen if you added a whole box of table salt to a glass of water? You need to know the solubility of salt to answer that question. The solubility of a substance is the amount of solute that dissolves in a given quantity of solvent at a specific temperature and pressure. If you add 36.2 grams of salt to 100 grams of water at 25°C, all of the salt will dissolve. Any extra salt will not dissolve—even if you stir the water for a long time. Why will the extra salt not dissolve? The figure shows a beaker containing a sodium chloride solution. Undissolved solid sodium chloride lies at the bottom of the beaker. You might expect all the solid particles to dissolve as water molecules interact with them. This does not happen. Particles do move from the solid into the solution, however dissolved particles also move from the solution back into the solid. These two process occur at the same rate when the solution is saturated. A saturated solution contains the maximum amount of solute for a given quantity of solvent at a constant temperature and pressure. If you add more solute to a saturated solution, it will not dissolve. An equilibrium, or balance, exists in a saturated solution between the solution and the undissolved solute under given conditions. An unsaturated solution contains less solute than a saturated solution does. You can add solute to an unsaturated solution and the solute will dissolve until the solution becomes saturated. a. Explain what is meant by the term “equilibrium” when applied to a saturated solution. b. What could you do to change a saturated solution to an unsaturated solution? c. The reading does not mention a supersaturated solution. How could you turn a salt water solution into a supersaturated solution? Learning Target B: Solubility Curves Use the solubility curve to answer the questions. 1. What four solutes are shown on the graph? 2. What is the solvent for all four solutes? 3. In what units is solubility measured? 4. What temperature range is shown? 5. For which solute(s) does solubility increase with temperature? What does this indicate about the identify of this/these solutes? 6. For which solute(s) does solubility decrease with temperature? What does this indicate about the identify of this/these solutes? 7. How many grams of Sodium Nitrate (NaNO3) could be dissolved in 300g of water at 50°C? 8. Ammonia, (NH3) is often used as a cleaning fluid. In order to make the strongest possible solution of ammonia (a solution containing a large amount of solute) would you use cold or hot water? Support your reasoning with evidence from the graph. 9. A solution of Potassium Nitrate (KNO3) contains 100 g of solute in 100g of water at 20°C and no solute is visible. Would you describe this as an unsaturated, saturated, or supersaturated solution? Provide evidence from the graph to support your response. 10. Use the graph to create a question of your own that could be asked about the solubility of one of the solutes. Write a good one and you may see it on the quiz .