Diluting Solutions to Prepare Workable Solutions

Making solutions of any concentration from a more concentrated source is possible. What does concentration mean? It's the amount of substance that exists in a given volume of solution.

Don't get it? Think of concentration as orange juice! Just that one can of orange juice has a high concentration. But then adding the 3 cans of water will make it diluted making it have a lower concentration.
A concentrated solution has a relatively high concentration meaning it has a large amount of substance dissolved in the solution.   
Dilute solutions have relatively low concentration so very little substance dissolved in the solution. These dilute solutions are usually formed when large amounts of solvent (usually water)  is added to a concentrated solution to produce a lower concentration.
Moles of solutes are constant. The only difference is that there's more water in the less concentrated solution. Therefore...

moles of solute before = moles of solute after

In terms of molarity & volume in L...

M1L1 = M2L2

Subscript 1= before & subscript 2= after.

Ex. What volume of 6.00 M HCl is used to make up 2.00L of 0.125 HCl
Remember the equation from above in bold purple! 
Rewrite the equation to fit with the information you have..so it'd be:
L1= M2 x L2  --> 0.125 M x 2.00 L = 0.0417 L
           M1                     6.00 M

Ex. If  1 drop (0.050 mL)  of 0.20 M NaBr is added to 100.00 mL of water, what's the molarity of NaBr in the resulting solution?
0.20 M x 0.050 mL= 1.0 x 10^-4 M
(100.00 + 0.050)mL
Remember when answering the questions to round to the correct amount of sigfigs!

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