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Behavior of Molecules in Solution

Behavior of Molecules in Solution. The state a substance is in at a particular temperature and pressure depends on two factors Kinetic Energy of the Particles Strength of the attraction between the particles. IMF. IMF = Intermolecular Forces Attractive forces between molecules.

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Behavior of Molecules in Solution

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  1. Behavior of Molecules in Solution

  2. The state a substance is in at a particular temperature and pressure depends on two factors • Kinetic Energy of the Particles • Strength of the attraction between the particles

  3. IMF • IMF = Intermolecular Forces • Attractive forces between molecules Much weaker than chemical bonds withinmolecules

  4. Overcoming Bonding Forces • IMF control how molecules bond together • Depending on the state of matter, molecules behave differently • In order for a molecule to change state (i.e. liquid to solid) the IMF of the molecules must be overcome. • The kinetic energy of the molecules need to overcome the IMF in order to change state ---Remember *What is kinetic energy??

  5. Overcoming Bonding Forces • IMF can be determined by the properties of the atoms/molecules. • Boiling Point (BP) • Melting Point (MP) • Vapor Pressure (VP) • Higher BP,MP,VP = stronger IMF

  6. A Model of the Dissolving of NaCl • Water is such a versatile solvent that it is sometimes called the universal solvent. • Its ability to act as a solvent is one of its most important physical properties.

  7. Like Dissolves Like • Although water dissolves an enormous variety of substances, both ionic and covalent, it does not dissolve everything. • The phrase that scientists often use when predicting solubility is “like dissolves like.” • The expression means that dissolving occurs when similarities exist between the solvent and the solute.

  8. Concentrated Versus Dilute • Chemists never apply the terms strong and weak to solution concentrations. • Instead, use the terms concentrated and dilute

  9. Preparing 1 L of an NaCl Solution • How would you prepare 1.0 L of a 0.15M sodium chloride solution? • First, determine the mass of NaCl to add to a 1.0-L container. • The 0.15M solution must contain 0.15 moles of NaCl per liter of solution.

  10. Preparing 1 L of an NaCl Solution • The proper setup, showing the conversion factors, is as follows.

  11. Preparing 1 L of an NaCl Solution = 8.8 g NaCl The result means you need to measure 8.8 g of NaCl, add some water to dissolve it, and then add enough additional water to bring the total volume of the solution to 1.0 L.

  12. Practice Problems • How would you prepare 5.0L of a 1.5M solution of glucose, C6H12O6? • You add 32.0 g of potassium chloride to a container and add enough water to bring the total solution volume to 955 mL. What is the molarity of this solution?

  13. Dilution M1V1=M2V2 M = MolarityV=Volume Ex: If I add 45 mL of water to 325 mL of a 0.15 M NaOH solution, what will the molarity of the diluted solution be?

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