Properties of Solutions
- 2. Parts of Solutions Dissolving is the process of mixing one substance into another to form a solution.
- 3. Parts of Solutions Dissolving is the process of mixing one substance into another to form a solution.
- 4. Parts of Solutions A solution is made up of a solvent and solutes. Generally, the solvent is the substance that exists in the greatest quantity in a solution. All other substances in a solution are solutes. solute solvent
- 5. Parts of Solutions A solution is made up of a solvent and solutes. Generally, the solvent is the substance that exists in the greatest quantity in a solution. All other substances in a solution are solutes. 78% Nitrogen 21% Oxygen 1% other substances solvent solute
- 6. Types of Solutions State of Solution Solid Liquid Gas Solvent is: Solutes can be: Solid gas or solid (called alloys) A saxophone is a solid solution of solid copper and solid zinc. Liquid solid, liquid, and/or gas Soda is a liquid solution of liquid water, gaseous carbon dioxide, and solid sugar and other flavorings. Gas gas A gaseous mixture of gaseous argon and gaseous mercury produces the light you see in many brightly colored signs.
- 7. Water as a Solvent In nature, water almost always exists as a solution. Why does nearly all water on Earth contain dissolved solutes? The answer has to do with the structure of the water molecule. Water is POLAR.
- 8. Water as a Solvent Water is often called the universal solvent because it dissolves many different substances. Polar solvents dissolve polar solutes easily. Nonpolar solvents dissolve nonpolar solutes easily. Because water is a polar solvent, it dissolves most polar and ionic solutes.
- 9. Concentration - How much is dissolved? Concentration is the amount of a particular solute in a given amount of solution.
- 10. Concentration - How much is dissolved? The terms concentrated and dilute are one way to describe how much solute is dissolved in a solution. These terms don’t state the exact amount of solute dissolved. One person might think that a solution is concentrated while another thinks it is dilute. concentrated! dilute!
- 11. Concentration - Describe using Quantity To calculate concentration for a solid dissolved in a liquid, you must know both the mass of solute (solid) and the volume of solution that contains this mass, and then, divide the mass of solute by the volume of solution.
- 12. Concentration - Describe using Quantity Suppose you want to calculate the concentration of salt in a 0.4 L can of soup. The label says it contains 1.6 g of salt. What is its concentration in g/L? In other words, how much salt would 1 L of soup have? 1.6g 0.4L = 4 g/L
- 13. Concentration - Describe using Quantity What is the concentration of 5 g of sugar in 0.2 L of solution? 5g = 0.2L 25 g/L
- 14. Concentration - Describe using Quantity How many grams of salt are in 5 L of a solution with a concentration of 3 g/L? xg 5L = 3 g/L x = 15 grams
- 15. Concentration - Percent Per Volume For solutions that contains liquids or gases as the solute, concentration of the solution is stated as the volume of solute in a given volume of solution. In this case, the units of volume must be the same—usually mL or L. Because the units match, you can state the concentration as a percentage.
- 16. Concentration - Percent Per Volume To calculate percent by volume, first divide the volume of solute by the total volume of solution. Then multiply the quotient by 100. For example, if a container of orange drink contains 3 mL of acetic acid in a 1,000-mL container, the concentration is 0.3 percent. 3 mL ÷ 1,000 = 0.003 0.003 x 100 = 0.3%
- 17. Solubility - How much will dissolve? What happens if you put a lot of sugar into a glass of water? Not all of the sugar dissolves. You stir and stir, but some sugar still remains at the bottom of the glass. That is because there is a limit to how much solute (sugar) can dissolve in a solvent (water).
- 18. Solubility - How much will dissolve? Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a given temperature and pressure. If a substance has a high solubility, more of it can dissolve in a given solvent.
- 19. Solubility - How much will dissolve? A saturated solution is a solution that contains the maximum amount of solute the solution can hold at a given temperature and pressure. An unsaturated solution is a solution that can still dissolve more solute at a given temperature and pressure.
- 20. Factors that affect how much can dissolve Temperature The solubility of sugar in water increases as the temperature of the water increases. This is true for many solid solutes. Some solids are less soluble in warmer liquids than in cooler ones. The difference depends on the chemical structure of the solid.
- 21. Factors that affect how much can dissolve Temperature How does temperature affect the solubility of a gas in a liquid? Let’s consider soda. More carbon dioxide bubbles out when you open a warm can of soda than when you open a cold can. Why? This is because the solubility of a gas in a liquid decreases when the temperature of the solution increases. Why?
- 22. Factors that affect how much can dissolve Temperature This is because the water molecules will be moving faster at higher temperatures. This movement will bump the gas out of the solution, therefore decreases solubility.
- 23. Factors that affect how much can dissolve Pressure What keeps carbon dioxide dissolved in an unopened can of soda? In a can, the carbon dioxide in the space above the liquid soda is under pressure. This causes the gas to move to an area of lower pressure—the solvent. The gas moves into the solvent and forms a solution. When you open the can, this pressure is released, and the carbon dioxide gas leaves the solution. Pressure does not affect the solubility of a solid solute in a liquid.
- 24. How fast a solute dissolves If solute and solvent particles come into contact more often, the solute dissolves faster. You can increase the contact between solvent and solute particles by: stirring the solution crushing the solute into smaller particles (increase surface area) heating a solution