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Warm-up

Warm-up. Using the Ideal Gas Law, calculate the mass of sulfur dioxide gas in a 350.0 mL flask at 780.0 Torr and 65.0 C. Solutions. Parts of a solution Solute - gets dissolved Solvent - does the dissolving (larger volume) soluble capable of being dissolved

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Warm-up

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  1. Warm-up Using the Ideal Gas Law, calculate the mass of sulfur dioxide gas in a 350.0 mL flask at 780.0 Torr and 65.0 C.

  2. Solutions • Parts of a solution • Solute- gets dissolved • Solvent- does the dissolving (larger volume) • soluble • capable of being dissolved • solid gradually disappears as particles leave the crystal and mix with water

  3. Electrolytes • Strong Electrolytes • completely create ions in water • conducts electricity • Weak Electrolytes • only partially create ions in water • partially conducts electricity • Nonelectrolytes • create no ions in water • do not conduct electricity

  4. Strong Electrolytes • Ionic compounds • Strong Acids: HCl, H2SO4, HNO3, HClO4 HBr, HI • Strong Bases: Family 1 + OH- and family 2 Calcium and down + OH-

  5. How ions are made • Dissociation • when an ionic compound breaks apart into its individual ions in water • Ca(NO3)2 Ca2+ + 2NO31- • Ionization • when a molecular compound creates ions in water • happens only when the bond is weak • HCl  H+ + Cl-

  6. How to increase the rate of solution • Surface area • Agitation (stirring) • Heating

  7. Solubility • Solubility- the amount of solute that can dissolve in a solvent at a certain temperature • depends on the characteristics of solute, solvent and temperature

  8. Solutions can be . . . • Saturated • solution that contains the maximum amount of dissolved solute • if more solute is added, it will fall to the bottom and not dissolve • Unsaturated • solution that contains less than the maximum amount of solute • Supersaturated • solution that contains more than the maximum amount of solute • can be created by heating up a solution and dissolving as much solute as possible • must allow it to cool undisturbed • will recrystallize quickly if seed crystal is added

  9. Supersaturated Solution

  10. Temperature and Solubility • Gases: • Increasing temperature usually • decreases gas solubility • Solids • Increasing temperature usually • increases solid solubility

  11. Heating Curve

  12. Pressure and Solubility • Little effect on solubility of liquids and solids • Increase in Pressure increases solubility of gases in liquids

  13. Pressure and Solubility

  14. Gas Pressure and Solubility

  15. Concentration- Measure of the amount of solute in a given amount of solvent or solution

  16. Molarity • is most often used to specify the concentration of a solution • number of moles of solute in one liter of solution • units: moles/liter = M

  17. Example 1 • 21.0 g of NaOH is dissolved in enough water to make 500. mL of solution. What is the Molarity?

  18. 3.4 g of KCl is dissolved in a 4.5 M solution. What is the solution’s volume

  19. Molarity by dilution • M1V1 = M2V2 • How much concentrated sulfuric acid (18M) is needed to prepare 650 mL of a 4.0M solution?

  20. To what volume should 50.0 mL of 15 M nitric aced be diluted to prepare a 5.0 M solution?

  21. Molality-number of moles of solute per kg of solvent • units: moles/kilogram = m

  22. What is the molality of a solution when 450 g of NaCl is dissolved in 2 Kg of water?

  23. What is the mass of KNO3 in a 2.5 m solution with a solvent mass of 1.5 Kg

  24. Effects of solute in pure solvent( Colligative properties) • Increase in boiling point • Decrease in freezing point • Decrease vapor pressure

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