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Understanding Solubility and Solutions: Key Factors and Types

Explore the properties of solutions and essential questions about solubility factors, concentration, and types of solutions. Learn about the impact of factors like nature of solvent, pressure, temperature on solubility. Discover the different types of solutions - unsaturated, saturated, supersaturated. Practice problems and examples help reinforce the concepts of solutes, electrolytes, and concentration measurements. Enhance your knowledge of chemistry with this comprehensive guide!

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Understanding Solubility and Solutions: Key Factors and Types

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  1. Properties of Solutions

  2. Essential Questions • What factors affect the solubility of solutions?

  3. Review • Solute: • Solvent: • Solution

  4. Review • Solute: one being dissolved • Solvent: one doing the dissolving • Solution: the solute and the solvent put together

  5. Factors Affecting Solubility • Nature of the Solvent • Polarity: “like dissolves like” • Polar with polar, Nonpolar with nonpolar • Pressure • Gas solutes only: increasing pressure will increase solubility • Carbonated beverages

  6. Factors Affecting Solubility Cont. • Temperature • Solids & Liquids: increasing temp. will almost always increase solubility • Gases: increased temp will decrease solubility

  7. Rate of Solution • Make a hypothesis as to which will dissolve faster, a sugar cube or granulated sugar. The amount of sugar is equivalent in each. Provide an explanation for your hypothesis.

  8. Factors Affecting Rate of Solution • Size of Particle • Increased surface area (smaller particles) allows greater contact with solvent • Amount of solute already dissolved • higher conc. slower rate

  9. Factors Affecting Rate of Solution Cont. • Temperature • Solids and Liquids: Increased temp. increases rate of solution • For Gases: Increased temp. decreases rate of solution • Stirring

  10. Types of solutions • Unsaturated: • Saturated: • Supersaturated:

  11. Types of solutions • Unsaturated: solute has not reached the saturation point yet (More solute can be added) • Saturated: saturation point has been reached, but no excess solute appears. • Supersaturated: Too much solute is present than can be dissolved. Excess solute is present.

  12. Think! • What would happen if you added more solute to a saturated solution?

  13. Solubility Curve

  14. Practice Problems • Use the solubility chart on the slide above to answer the following. • What amount of NaCl is needed to make a saturated solution at 80oC? 2. What type of solution exists when 90g KNO3 is dissolved at 40oC?

  15. Think: • What would happen if you added more solute to a saturated solution?

  16. Solute Types • Electrolytes • Non-electrolytes

  17. Types of Solutes • Electrolytes • Break apart into ions in solution • Number of ions = Subscript total • Conduct electricity • Example: NaCl in solution

  18. Types of Solutes Cont. • Non-electrolytes • Stay whole in solution • Do not conduct electricity • Example: CO2

  19. Types of Solutes Cont. • Type of solute affects the total # of solute particles in solution • Ex: If one had equal concentrations of KBr, an electrolyte and C6H12O6, a nonelectrolyte in solution, there would be more particles in the KBr solution.

  20. Examples • Determine the number of particles in the following: • NaCl, an electrolyte • NO2, a non-electrolyte • CH4, a non-electrolyte • CaCl2, an electrolyte

  21. ESSENTIAL QUESTION • How “strong” is that solution? • Think-ink-share…. • What is this lesson about? What do we mean by a solution being strong? • Give me a synonym for the word “strong” as it is meant in the EQ.

  22. Concentration • Measured in molarity • Think…. How is concentration measured? http://www.youtube.com/watch?v=tXG0PACMUOo The more you add… the more concentrated. The less volume you have, the more concentrated.

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