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Solution Chemistry

Solution Chemistry. Warm-Up 2/8/17. Solutions are all around us, can you think of what some solutions are?. Some Examples. Definition. Solutions are homogeneous mixtures that contain two or more substances. Solutions consist of solutes and solvents.

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Solution Chemistry

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  1. Solution Chemistry

  2. Warm-Up 2/8/17 Solutions are all around us, can you think of what some solutions are?

  3. Some Examples

  4. Definition Solutions are homogeneous mixtures that contain two or more substances. Solutions consist of solutes and solvents. Solutesare the dissolved substance in a solution. Solventsare the dissolving medium in a solution. Solute Solvent

  5. Solutions Even though most solutions are liquid, solutions do exist as solids, liquids, and gases. Gases: Air Solid Alloys Liquids

  6. Soluble versus Insoluble Some substances readily combine to form solutions, others do not. A substance that dissolves in a solvent is said to be soluble. A substance that will not dissolve in a solvent is said to be insoluble. Salt and Water Soluble Sand and Water Insoluble

  7. Miscible versus immiscible When a liquid dissolves in another liquid it is said to be miscible. Immiscible is when two liquids don’t dissolve. Oil and Water: Immiscible Water and alcohol: Miscible

  8. Concept Check What is the difference between soluble and miscible? How are they similar? Write this down in your notebook.

  9. Solvation Solvation is the process of dissolving. Solute particles are surrounded by solvent particles. Solute particles are separated and pulled into solution.

  10. Concept Check Will KF undergo solvation in water? Why or why not? If it does, describe what will happen.

  11. Warm-Up 2/9/17 Get out half a sheet of paper and write and answer the following question: Will NaF undergo solvation? Why or why not? If yes, explain the process.

  12. The substance dissolved in a solution is the: • Mixture C) Solvent • Solute D) Solution

  13. What is the processes of dissolving? • Mixture C) Solvation • Solvent D) Solution

  14. When a liquid dissolves in another, it is said to be • Soluble C) insoluble • Immiscible D) miscible

  15. Electrolytes A solution is said to be an electrolytewhen the solution conducts electricity. This happens when there are charged particles in the solution.

  16. Electrolytes There are three types: Non-electrolyte- when the solution does not conduct electricity Weak electrolyte- when the solution conducts some electrical current (but not a lot) Strong electrolyte- when the solution conducts electricity

  17. Electrolytes (Continued) Strong electrolytes are ionic compounds. Weak or non-electrolytes are covalent compounds. ethanol NaCl Acetic acid

  18. Solubility Unsaturated solution More solute dissolves Saturated solution No more solute dissolves Supersaturated solution Unstable solution and crystals form

  19. Supersaturated Solutions Diet coke and Mentos Heat Packs

  20. Concentrated and Dilute A concentrated solutioncontains more solute than solvent A dilute solutioncontains more solvent than solute

  21. Concept Check Explain the difference between a supersaturated solution and an unsaturated solution. Give an example of each.

  22. When a relatively small amount of solute is dissolved in a solution, it is said to be: • insoluble C) dilute • concentrated D) immiscible

  23. A substance that dissolves in water to give a solution that does not conduct an electric current: • electrolyte C) solvation • concentrated D) non-electrolyte

  24. Solubility Trends Solids • Solubility of most solids increase with temperature (the higher the temp, the faster the solid dissolves. • Solids dissolve quicker with increasing surface area of the solid (the smaller the size, the faster it dissolves) • Stirring will help dissolve the solid faster

  25. Solubility Trend (Cont.) Gases • Solubility of gases decreases with increasing temperature (the colder the temp, the faster the gas dissolves) • Solubility of gases increases with pressure (higher the pressure, the more the gas will dissolve)

  26. Math Time! Concentration of a solution has 4 main 1. Molarity (M) M= moles liters 3. Percent composition a) %mass/volume = mass of solute X100 %m/v volume of solution b) % volume/volume = volume of solute X100 %v/v volume of solution measurements: 2. Grams per Liter g/L = grams liters 4. Parts per million ppm= mass of solute X106 mass of solution

  27. Problems on Molarity If you have 2 moles of glucose in 8 liters of solution, find the molarity of the solution. Equation: M=moles liters 2 moles = 0.25 M 8 liters

  28. Problems on Molarity A salt solution has a volume of 250 mL and contains 0.70 moles of NaCl. What is the molarity?

  29. Problems on Molarity A saline solution contains 0.90 grams of NaCl per 100 mL of solution. What is the molarity?

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