SOLUTIONS UNIT CORRECTIVES
Skill 1: Read pages 467 – 470
Helpful video: https://webertube.com/video/18053/solutions
1. Define solution, solute, solvent, alloy, tincture
2. Name the solute in (a) salt water, (b) ammonia water, (c) water vapor in air, (d) a brass alloy containing 75% copper and 25% zinc, (e) 40% alcohol solution, and (f) tincture of iodine.
3. Define and state one example of a (a) gaseous solution, (b) liquid solution, (c) solid solution.
4. In what way does a solution behave different from a suspension when a beam of light is shined at it?
5. What are the properties of a solution?
Skill 2: Read pages 470 - 473
1. Define solubility and polarity
2. Describe the process by which a solute is able to dissolve in a solvent.
3. Why can’t benzene dissolve sodium chloride? Remember sodium chloride will dissolve in water.
4. How does a rise in temperature affect the solubility of (a) most solid solutes, (b) all gases?
5. The caps are removed from a warm and a cold bottle of a carbonated beverage. The cold soda bubbles only slightly. There are many more bubbles in the warm soda. Explain the difference.
6. What are several things that could be done to dissolve a large quantity of solute as quickly as possible?
Skill 3: Read section 15.2 page 472
1. Define solubility, unsaturated solution, saturated solution, and supersaturated solution.
Use the graphs on the third page to answer questions 2-6.
2. Find the solubility of NH3 at 50oC.
3. What is the solubility of KClO3 at 90oC?
4. How many more grams of sodium nitrate can be dissolved in 100 grams of water at 60 oC, than potassium nitrate at the same temperature?
5. 40 grams of potassium chloride is dissolved in 100 grams of water at 80 oC. Other than removing some of the water, what are TWO things that can be done to make this a saturated solution?
6. How many grams of ammonium chloride can be dissolved in 400 grams of water at 80 oC?
Skill 4: Read page 472 and 476
Solution concentration simulation - http://phet.colorado.edu/en/simulation/concentration
1. Define dilute, concentrated, saturated, soluble, and molarity.
2. Silver sulfate is only slightly soluble in water. Explain why the following solutions can or cannot be prepared using silver sulfate as the solute? (a) dilute solution, (b) concentrated solution, (c) saturated solution.
3. A beaker contains a solution made of a solid completely dissolved in a liquid solvent. For each of the following actions, state whether it will (1) always, (2) sometimes, or (3) never make the solution more concentrated. Explain. (a)Raise the temperature of the solution. (b)Add more solute. (c) Add more solvent. (d) Stir the solution vigorously.
(Over)
4. Draw a diagram of three containers with a liquid solution in them. Use dots to represent the solute. Solution A is twice as concentrated as solution B both have the same volume. Solution C has the same concentration as solution A but with twice the volume of solution A.
Skill 5: Read page 474 – 481
Helpful video: https://webertube.com/video/21820/solution-preparation
Helpful video: https://webertube.com/video/18144/solution-concentration-calculations
1. Define molality, percent by mass, and density, acid, base
2. A solution that is labeled “0.150 M NaOH” would contain ______mole of NaOH per liter of solution.
3. An alcoholic iodine solution (tincture of iodine) is prepared by dissolving 5.15 g of iodine crystals in enough alcohol to make 225 mL of solution. Calculate the molarity of the solution.
4. Describe the conditions necessary to have an acidic solution, describe this in terms of the pH and the concentration of hydrogen ions compared to hydroxide ions.
5. How many moles of potassium thiocyanate, KSCN, are dissolved in 320 ml of a 0.250 molarity solution? How many grams of KSCN are in this solution?
6. An experiment is performed in which the solvent is evaporated form a solution leaving the solute behind. Use the data below to calculate the density, molality, molarity and percent by mass of the solute in the solution.
Volume of the solution = 75.0 ml
Mass of the evaporating dish = 85.56 g
Mass of the evaporating dish and the solution = 192.83 g
Mass of the evaporating dish and the solute (barium hydroxide) = 94.88 g
Skill 6: Read pages 495 – 496
pH simulation - http://phet.colorado.edu/en/simulation/ph-scale
1. Define osmosis, freezing point depression, and molality.
2. Antifreeze that you use in your car could also be called “antiboil”. Explain why.
3. A solution has a molality of 1.00 mole/kg. The solvent in this solution has a boiling point elevation constant of 2.53oC/molality. What will be the difference between the boiling point of this solution and the boiling point of the pure solvent?
4. A solution is prepared by adding 472 g of C2H4(OH)2 to 1500.0 grams of water. What is the freezing point of the solution?
5. What determines which way water moves by the process of osmosis?