DILUTION OF SOLUTION

In the previous lesson, we talked about Molarity, now... We are talking about the Dilution of Solution.. ( Super!! ) 

Chemicals are usually shipped in a concentrated mode. So to make it less concentrated, water is usually added!!

In this lesson, we are going to learn to make solutions of any concnetration from a more concentrated source. 

You guys remember the law of conservation of mass, right?? ..... Yeah I didn't think so either..

Basically, the amount of mass enterring a reaction is equal to the amount of mass coming out!! How is this relevant, you may ask? Well , one answer... Moles of a solute are constant, and do not change..

The simple equation for this is derived from the previous lesson 

M1(L1) = M2(L2)

I have ...                                    I need...

         2.00 L    of HCl                          0.8 L

         16.0 M                                      2.0 M

Here comes the magic...

        16 x L1 = 2 x 0.8 

              L1 = 0.100 L

So you add 0.800 - 0.100 = 0.700 L of water to get the concentration you needed ..

THAT'S IT!!
see you next class !!!