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Solutions

Solutions. By Aimee Chavez. Becoming a solution. Any states of matter solid, liquid, gas can become part of a solution. To form , one substance must dissolve in another. Dissolving. Solution is a homogeneous mixture of two or more substances. Every solution has a solute and solvent .

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Solutions

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  1. Solutions By Aimee Chavez

  2. Becoming a solution • Any states of matter solid, liquid, gas can become part of a solution. • To form , one substance must dissolve in another.

  3. Dissolving • Solution is a homogeneous mixture of two or more substances. • Every solution has a solute and solvent. • The solution takes the state of the solvent.

  4. Types of solution

  5. Solute and Solvent Solute: substance whose particles are dissolved in solution. Solvent: the substance in which the solute dissolves. Gives the state of the solution i.e. solid liquid or gas A homogenous mixture of two or more substances.

  6. Three ways of dissolving • Solute and solvent particle must attract one another. • Solute attracts solute and solvent attracts solvent so the attractions that hold them together must be overcome.

  7. Dissociation • Process in which an ionic compound separates into ions as it dissolves. • NaCl is an ionic compound. Water is a polar molecule, and is attracted to the ions in the solute. • The crystal dissolves as the Na and Cl ions are pulled into solution, one by one

  8. Dispersion in Molecular Compounds • Sugar dissolves in water by dispersion, or breaking into small pieces that spread throughout the water. • Both sugar and water are polar molecules, so they attract one another. The water molecules are constantly moving, they collide with the sugar crystals. Attractions form between the water and sugar . When enough water has surrounded a sugar molecule , the attractions between them are great enough to overcome the attractions holding the sugar molecule to the surface of the crystal. The sugar molecule breaks free, and is pulled into solution by the water molecules.

  9. Ionization of Molecular Compounds • HCl is a molecular compound in which a H and a Cl share a pair of electrons. When HCl dissolves in water , the H electron from each HCl is transferred to a water molecule. For each HCl a hydronium ion H³O+ and a Chloride ion Cl- are produced. • The process in which neutral molecules gain or lose electrons is know as ionization. • A chemical change (2 new substances)

  10. Solids from Solutions • Crystallization: a solute can come back out of it’s solution and form a solid. • Cooling or evaporating • Some solutions form a precipitate after a chemical change. • Stalactites and stalagmites

  11. Properties of Liquid Solutions • Conductivity: some substances such as sodium chloride will conduct an electric current because the ions are able to move freely.

  12. Freezing point and boiling point: adding a solute can decrease the freezing point. Example MgCl₂ on snowy roads. A solute can also raise the B.P. of the solvent. Example: coolant in car radiators

  13. Factors Affecting Rates of Dissolving • Depends on frequency and energy of collisions that occur between small particles. • 1. surface area: can increase but breaking, crushing or breaking up the solute. Increases amount of collisions in particles.

  14. 2. stirring: • : moved dissolved particles away from the surface and allows for more collisions.

  15. 3. temperature: • increasing temperature of solvent increases rate of dissolving. Causes particles to move faster. Both number of collisions and energy of these collisions with solute increase.

  16. solubility • The maximum amount of solute that dissolves in a given amount of solvent at a constant temperature. • Expressed as grams of solute per 100 gm. of solvent at a specified temperature. • Table salt 36.0 g per 100 g water at 20°C • Table sugar 203.9 g per 100 g water at 20°C

  17. Classifying solutions • Saturated: a solution that contains as much solute as the solvent can hold at a given temperature. • Unsaturated: a solution that has less than the maximum amount of solute that can be dissolved • Supersaturated: a solution that contains more solute than it can normally hold at a given temperature.

  18. Red Blood Cells in our body and Plant cells

  19. Factors affecting solubility • 1. polar and non polar: like dissolves like

  20. 2. temperature: solubility of solids increases as the solvent temperature increases. Gases become less soluble as the temperature of the solvent increases.

  21. 3. pressure: increasing pressure of gas increases its solubility in a liquid. CO₂ under pressure in a sealed can of soda.

  22. concentration • The amount of solute dissolved in a specified amount of solution. • Can be expressed as percent per volume or percent per mass. • Percent by volume or mass = volume or mass of solute /volume or mass of solution x 100 %

  23. Acids & Bases Foldable

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