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Solution Concentration

Solution Concentration. Section 14.2. Concentration - amount of solute dissolved in a specific amount of solvent. concentrated - a lot of solute dilute - very little solute. Percent mass = mass of solute x100 mass of solution.

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Solution Concentration

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  1. Solution Concentration Section 14.2

  2. Concentration - amount of solute dissolved in a specific amount of solvent concentrated - a lot of solute dilute - very little solute

  3. Percent mass = mass of solute x100 mass of solution Example #1 - In order to maintain a sodium chloride solution similar to ocean water, an aquarium must contain 3.6g of NaCl per 100.0g of water. What is the % mass NaCl of the solution?

  4. Percent mass = mass of solute x100 mass of solution % = 3.6 g x100 103.6g = 3.5% Mass of solute + mass of solvent

  5. Percent (m/v) = mass of solute x100 volume of solution (in mL) Example #2 – How many grams of solute are needed to prepare 2.00L of 2.00% glucose (m/v)

  6. 2.00% = g x100 2000mL = 40.0 g x1

  7. Molarity (M) = moles solute liters of solution Example #3 - A 100.5 mL intravenous solution contains 5.10g of glucose (C6H12O6). What is the molarity of this solution?

  8. Molarity (M) = moles solute liters of solution mol C6H12O6 5.10g C6H12O6 1 x __________ 180.16 g C6H12O6 = 0.0283 mol = .1005 L 100.5 mL

  9. M = 0.0283 mol 0.1005 L = 0.282 mol/L or M x3

  10. Example #3 - how would you prepare 2.00L of a 5.0M NaCl solution? 5.0 = mol 2.00 L = 10. mol 10. mol NaCl 58.443 g NaCl x __________ 1 mol NaCl

  11. = 580 g NaCl * to make the solution dissolve 584 g of NaCl in enough water to make 2.00 L of solution x1

  12. Diluting Solutions - using a concentrated solution to make a diluted solution M1V1 = M2V2

  13. Example #4 - what volume, in milliliters, of 2.00 M calcium chloride stock solution would you use to make 0.50 L of 0.300M solution? M1V1 = M2V2 (2.00)(V1) = (.300)(.50) 0.075L = 75 mL V1 = (0.300)(0.50L) (2.00) V1 = 0.075L

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