Solution Preparation and Dilutions Solution Preparation How do
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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 Add enough solvent to reach the desired volume.
Example 1: Prepare a 6 L solution of 4 M Na. Cl
Example 2: Prepare a 250 ml solution of 0. 05 M HCl
Example 3: Prepare a 400 ml solution of 5 M Cu. SO 4
Dilutions
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 M 1 V 1 = M 2 V 2 Used when 2 solutions are involved Units do not matter but keep the same units throughout the problem !!! Ex. Tea and sweetner
Example 1: Prepare 2. 50 L of a 0. 360 M H 2 SO 4 solution from a stock H 2 SO 4 solution of 18. 0 M.
Example 2: A stock solution of KF has a concentration of 1. 20 M. To what final volume must 100 ml of this solution be diluted to produce a 0. 45 solution of KF?
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 500 ml of a 2. 4 M KCl solution to make a 1. 0 M solution?
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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- Domain 1
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- Domain 1: planning and preparation examples