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Solutions

Solutions. Solution – _________________________________ ____________________________________________________________________________________ Solute – _________________________________ ____________________________________________________________________________________

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Solutions

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  1. Solutions • Solution – _________________________________ ____________________________________________________________________________________ • Solute – _________________________________ ____________________________________________________________________________________ • Solute – _________________________________ ____________________________________________________________________________________

  2. Polar and Nonpolar Solvents • A liquid composed of polar molecules is a polar solvent. Water and ethanol are polar solvents. • A liquid composed of nonpolar molecules is a nonpolar solvent. Hexane is a nonpolar solvent.

  3. Like Dissolves Like • ________________________________________ • ________________________________________ • ________________________________________ • Methanol dissolves in water, but hexane does not dissolve in water. • Hexane dissolves in toluene, but water does not dissolve in toluene.

  4. Polar and Nonpolar Solvents

  5. Miscible & Immiscible • Two liquids that completely dissolve in each other are __________________ liquids. • Two liquids that are not miscible in each other are _______________________liquids.

  6. Miscible & Immiscible • Polar water and nonpolar oil are immiscible liquids and do not mix to form a solution.

  7. Solids in Solution • When a solid substance dissolves in a liquid, the solute particles are attracted to the solvent particles. • When a solution forms, the solute particles are more strongly attracted to the solvent particles than other solute particles.

  8. Solutions 23.00 grams of hydrogen chloride is added to 55.00 grams of water. solvent = solute = solution =

  9. Solutions A potassium permanganate solution contains 1.223 grams of solute solution = solvent = solute =

  10. Solutions 59.88 mL of benzene has 12.4 mL of chloroform dissolved into it. solvent = solute =

  11. Solids in Solution • ____________________________________ ____________________________________ ____________________________________ • ____________________________________ _____________________________________ _____________________________________

  12. Rate of Dissolving • There are three ways we can speed up the rate of dissolving for a solid compound: • ________________________: • ____________________________________________ ____________________________________________ • ________________________: • ____________________________________________ ____________________________________________ • ________________________: • ____________________________________________

  13. Saturated Solutions • A solution containing exactly the maximum amount of solute at a given temperature is a ____________ ____________________________________________ • A solution that contains less than the maximum amount of solute is an _______________________ ____________________________________________ • Under certain conditions, it is possible to exceed the maximum solubility of a compound. A solution with greater than the maximum amount of solute is a ________________________________________

  14. Supersaturation

  15. Concentration of Solutions • The concentration of a solution tells us how much solute is dissolved in a given quantity of solution. • There are several measurements for the concentration of a solution:

  16. Concentration – Mass Percent • Mass percent concentration compares the _____________________________________.

  17. Concentration – m/v Percent • Mass/volume percent concentration compares _____________________________.

  18. Concentration – Volume Percent • Percent by volume concentration compares the _______________________________________.

  19. Concentration – Mass Percent • A student prepares a solution from 5.00 g NaCl dissolved in 97.0 g of water. What is the concentration in m/m %?

  20. Concentration – Mass Percent What is the mass percent of a solution that is made up of 75.0 grams of lithium fluoride and 125 grams of water? given: asked:

  21. Concentration – Mass Percent What is the mass percent of a solution which weighs 625 grams and contains 100.0 grams of potassium bromide? given: asked:

  22. Concentration – Volume Percent What is the volume percent of a solution which contains 30.0 mL ethanol and 720.0 mL of water? given: asked:

  23. Solutions Solution – A system in which one or more substances are mixed or dissolved in another substance. Solute – The substance that is being dissolved, or the least abundant component, of a solution.

  24. ________ Percent Unit Factors • We can write several unit factors based on the concentration 4.00 v/v % ethanol:

  25. ________ Percent Unit Factors • We can write several unit factors based on the concentration 8.11% by mass (m/m) ethanol:

  26. Concentration – Molarity

  27. Avogadro’s # The mole Only 3 options of what to do with the mole: mole particles molar mass mole mass molar volume mole volume mole-to-mole ratio mole “X” mole “Y”

  28. Molarity Unit Factors • We can write 2 conversion factors based on the concentration 6.00 MNaOH:

  29. Concentration – Molarity How many moles of NaClare in 2.5 L of a 0.355 M solution of sodium chloride?

  30. Concentration – Molarity What volume of a 1.250 M potassium hypoiodite solution will contain 0.00456 moles of potassium hypoiodite?

  31. Concentration – Molarity How many grams of Li2CrO4are in 250.0 mL of 0.100 MLi2CrO4solution?

  32. Concentration – Molarity • What volume of 12.0 MHCl contains 9.15 g of HCl solute (36.46 g/mol)?

  33. Concentration – Molarity How would you make 0.0250 L of a 0.0998 M solution of rubidium carbonate (230.95 g/mol)?

  34. Solution Stoichiometry Problem What is the mass of all products and reactants after the following reaction finishes: 37.5 mL of 0.100 M aluminum bromide solution reacts with 80.1 mL of 0.133 M silver nitrate solution?

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