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Solution Preparation and Dilutions

Solution Preparation and Dilutions. Solution Preparation. How do we create chemical solutions in a laboratory setting with a certain concentration/molarity? Obtain the mass of the chemical compound serving as solute Dissolve the solute in a small amount of the solvent

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Solution Preparation and Dilutions

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  1. Solution Preparation and Dilutions

  2. Solution Preparation • How do we create chemical solutions in a laboratory setting with a certain concentration/molarity? • Obtain the mass of the chemical compound serving as solute • Dissolve the solute in a small amount of the solvent • Add enough solvent to reach the desired volume.

  3. Example 1: • Prepare a 6L solution of 4M NaCl

  4. Example 2: • Prepare a 250 ml solution of 0.05M HCl

  5. Example 3: • Prepare a 400 ml solution of 5M CuSO4

  6. Dilutions

  7. What is a dilution? • Taking a CONCENTRATED solution and making it LESS concentrated • Adding more solvent to decrease the amount of solute in the solution • M1V1 = M2V2 • Used when 2 solutions are involved • Units do not matter but keep the same units throughout the problem !!! • Ex. Tea and sweetner

  8. Example 1: • Prepare 2.50L of a 0.360M H2SO4 solution from a stock H2SO4 solution of 18.0 M.

  9. Example 2: • A stock solution of KF has a concentration of 1.20M. To what final volume must 100ml of this solution be diluted to produce a 0.45 solution of KF?

  10. Example 3: • What volume of 17.4 M acetic acid is needed to prepare 1.00 L of 3.00 M acetic acid? • How much water would I need to add to 500ml of a 2.4M KCl solution to make a 1.0M solution?

  11. Serial Dilutions • A type of dilution • The dilution is made through a series of smaller dilutions from a stock or original solution • Dilution factor • Amount transferred/(amount transferred + amount of water) • 1 ml of chemical solution into 9 ml of water is a 1/10 dilution factor. **How dilute is the resulting solution, multiply the dilution factors for each series.

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