making dilutions. diluting a solution reduces the number of moles of solute per unit volume, but the...
TRANSCRIPT
Making Dilutions
• Diluting a solution reduces the number of moles of solute per unit volume, but the total number of moles does not change.
• Higher molarity = more concentrated
Put in order from most dilute to most concentrated
• 6.0 M
• 0.05 M
• 1.05
• 1.5 M
• 5 x10-3 M
• 3.5 M
http://phet.colorado.edu/en/simulation/molarity
How can we change concentration?
• If we want to make 3.0 M hydrochloric acid, but we only have 6.0 M hydrochloric acid, what can we do?
Dilution Equation
• M1V1= M2V2
• Volumes can be in mL or L, but they must be the same on both sides.
• V is total volume of the solution, not the volume of water added!
Practice• I have 20.0 mL of 2.00 M solution. I need to make
0.400 M solution. To what volume should I add?
• M1V1= M2V2
• (2.00 M)(20.0) = (0.400 M)V2
• V2 = 100. mL
• I have 0.25 L of 3.0 M HBr. How much water should be added to produce a 2.0 M solution?
• M1V1= M2V2
• (3.0 M)(0.25 L) = (2.0 M)V2
• V2= 0.375 L
• V is total volume.
• I already have 0.25 L of HBr,
• 0.375 - 0.25 = 0.125
• So I should add 0.13 L of water