Solutions & Solubility Solution Preparation by dilution.
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Transcript of Solutions & Solubility Solution Preparation by dilution.
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Solutions & Solubility
Solution Preparation by dilution
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Review 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
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Preparing a Solution by Dilution Dilution = the process of decreasing
the concentration of a solution, usually by adding more solvent
Stock Solution = a solution that is in stock or on the shelf (i.e., available); usually a concentrated solution
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Equipment needed to prepare a standard solution: Graduated Pipettes and bulbs Volumetric flask
Solution Preparation
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Graduated & Volumetric Pipettes and Bulb transfer small quantities of liquid
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The Formula the number of moles (n) does not change
when more solvent is added to a solution; only the concentration changes
therefore, ni (initial) = nf (final)
If a solution is diluted from V1 to V2, the molar concentration of that solution changes according to the following equation: C1 V1 = C2 V2
** remember: n = C X V **
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The VariablesC1V1 = C2V2
C1 = initial concentration of stock solution
V1 = volume of stock solution to be transferred
C2 = final concentration of dilute solution
V2 = final volume of dilute solution
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Example How do you prepare 250 mL of a 0.01
mol/L solution from a stock solution of 0.1 mol/L? The Calculations: C1V1 = C2V2
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The Procedure Remove the calculated V1 amount of your
stock solution using a pipette. Place that volume into a clean, dry volumetric
flask of the volume needed for your diluted solution
Add distilled water to the mark of the volumetric flask
Label the flask with the new solution concentration
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Now you try…. Make 50.0mL of 0.150M NaCl solution from
your 0.300M stock solution