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Solutions & Solubility

This guide provides a comprehensive overview of preparing standard solutions from solids, primarily using sodium hydroxide as an example. It highlights the importance of standard solutions in research laboratories and industrial applications, emphasizing their role in chemical analysis and reactions. Detailed steps include calculating the number of moles and mass of solute needed, weighing the solid, dissolving it in distilled water, and transferring the solution to a volumetric flask. Essential equipment such as an electronic balance and volumetric flask is also discussed.

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Solutions & Solubility

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  1. Solutions & Solubility 6.5 Solution Preparation

  2. Solution Preparation from a solid • Standard Solution = a solution for which the precise concentration is known • Used in research laboratories and industrial processes • Used in chemical analysis and precise control of chemical reactions

  3. Solution Preparation • Equipment needed to prepare a standard solution: • Electronic balance • Volumetric flask

  4. Volumetric Flask

  5. Example • For an acid-base titration, you need to prepare 250 mL of a 0.50 mol/L sodium hydroxide solution

  6. Step 1 • Calculate the number of moles of solute needed.

  7. Step 2 • Calculate the mass of solute needed.

  8. Step 3: The Experimental Procedure Preparing a solution from a solid

  9. Experimental Procedure • Weigh out the required mass of sodium hydroxide in a clean beaker. • Dissolve the solid in 40 – 50 mL of distilled water • Rinse the beaker 2-3 times with small amounts of distilled water and transfer into the volumetric flask • Add distilled water to the flask until the volume is 250 mL • Stopper the flask and mix the contents thoroughly by repeatedly inverting the flask.

  10. Homework • Read pg. 300 – 302 • Do #1, 2, 4a, 5a on pg. 302

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