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Solutions and Solubility

Solutions and Solubility. Vocabulary. Dissociating = to break apart ions NaCl + H 2 O = Na+ separates from the Cl- and each are surrounded by water molecules Dissolving = to break apart molecules Sugar + H 2 O = molecules of sugar separate in water Ionizing = another term for Dissociation.

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Solutions and Solubility

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  1. Solutions and Solubility

  2. Vocabulary • Dissociating = to break apart ions • NaCl + H2O = Na+ separates from the Cl- and each are surrounded by water molecules • Dissolving = to break apart molecules • Sugar + H2O = molecules of sugar separate in water • Ionizing = another term for Dissociation

  3. Non electrolytes do not conduct electricity when dissolved in water. • Polar covalent molecules such as methanol CH3OH don’t fall apart into ions when they dissolve. • Weak electrolytes don’t fall completely apart into ions. • Strong electrolytes do ionizes completely.

  4. Solutions are composed of: • Solvent = does the dissolving; always in the greater concentration • Solute = is dissolved; always in lesser concentration solvent concentration > solute concentration Ex. 5g of NaCl + 1 Liter of water: • Solvent = • Solute =

  5. Types of Solutions: • Saturated Solution: undissolved solute is in equilibrium with the dissolved solute • Unsaturated Solution: contains less than the saturated amt. of solute for that temperature • Supersaturated Solution: contains more solute than a saturated solution can normally hold.

  6. Who will dissolve me? • “Like dissolves like” = polar solvent will dissolve polar solute or nonpolar solvent will dissolve nonpolar solute. • Ex. Salt will dissolve in water but not acetone. • Ex. Oil will not mix with water • Miscibility - the ability of two liquids to be mixed. • Oil is immiscible in water • Vinegar is miscible in water

  7. Rate of Solution Affected By: • Surface area of solid exposed to solvent. • Increase SA, increase solution rate • Stirring of solution • Stirring the solution will prevent buildup of saturated solution around solute • Kinetic Energy (motion) of solute and solvent • Increase T = increase KE = Increase solution rate

  8. Solubility • The maximum mass of a substance that will dissolve in 100g of water at a given temp. • Use solubility chart to determine. • EX: 40g of NaCl dissolves in 100g of water at 80oC.

  9. Solubility Curve • A solubility curve shows the maximum mass of solute that will dissolve in 100g of water from 0oC-100oC.

  10. Types of Solutions • Saturated Solution: undissolved solute is in equilibrium with the dissolved solute (on the line) • Unsaturated Solution: contains less than the saturated amt. of solute for that temperature (below the line) • Supersaturated Solution: contains more solvent than a saturated solution can normally hold. (above the line)

  11. 1. How many grams of potassium iodide can be dissolved in 100g of water at 700C? 2. 100g of sodium nitrate in 100g of water at 50oC is a(n) _______ solution. 3. 190 g of sodium nitrate in 100g of water at 80oC is a(n) _______ solution. 4. How many grams of potassium nitrate make a saturated solution at 70oC? 5. Describe an unsaturated solution of potassium chlorate.

  12. Molarity • Molarity = moles ---------------- Liters M1V1 = M2V2

  13. Molarity Practice Problems • Your lab requires 120 ml of a 3.0 M HCl solution. How many grams of HCl will you need for the solution? • What is the molarity of a solution in which 10.0 g of NaOH is dissolved in 450ml of solution?

  14. Na + Cl2 ---> NaCl • A) Balance the equation • B) If you begin with 20.7 g of sodium, what mass of sodium chloride will be produced? • C) What will be the molarity of a 450ml sodium chloride solution containing the mass of sodium chloride found in B above?

  15. Molarity A X ml A = Molarity B X ml B • To what volume should 25 ml of 15M nitric acid be diluted to prepare a 3.0 M solution? • What volume of concentrated 18M sulfuric acid is needed to prepare 250ml of a 6.0M solution?

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