Presentation on theme: "Taking a concentrated solution and making it less concentrated."— Presentation transcript:
Taking a concentrated solution and making it less concentrated
Diluting a solution A solution is made when a solute is dissolved in a solvent A dilute solution contains a little solute and a lot of solvent. Example: orange juice concentrate 10 cans of water(yuck!) A concentrated solution contains a lot of solute and a little solvent. Example: orange juice concentrate with only ½ can of water Perfect orange juice: 1 can of concentrate (solute) and three cans of water (solvent)
Diluting a Solution Making Dilutions To dilute a solution, more solvent is added to a concentrated solution Dilution formula: M 1 V 1 = M 2 V 2 M 1 = the molarity of the concentrated solution V 1 = the volume of the concentrated solution needed for the dilution M 2 = the desired molarity of the dilute solution V 2 = the desired volume of the dilute solution
Diluting a solution To make the dilution, measure the quantity of the concentrated solution needed, place it in a volumetric flask, and add enough water to make the TOTAL volume of the desired dilute solution.
Diluting a Solution Example: How many mL of a 1.0 M NaCl solution is needed to make 250 mL of a 0.20 M NaCl solution? M 1 = 1.0 M M 2 = 0.20 M V 1 = ? V 2 = 250 mL V 1 = M 2 V 2 = (0.20 M)(250 mL) = 50. mL of 1.0 M NaCl M 1 1.0 M
Diluting a Solution Example: How would you prepare 525 mL of a 0.15 M Ca(NO 3 ) 2 solution if you have 2.0 L of a 2.0M Ca(NO 3 ) 2 solution available. M 1 = 2.0 M M 2 = 0.15 M V 1 = ? V 2 = 525 mL V 1 = M 2 V 2 = (0.15 M)(525 mL) = 39 mL of 2.0 M Ca(NO 3 ) 2 M 1 2.0 M Add 39 mL of 2.0 M Ca(NO 3 ) 2 to enough water to make 525 mL of solution