If 40.0 mL of a #3.0x10^(-5)# solution is diluted to 100 mL, what is the resulting concentration?

1 Answer
Aug 26, 2016

Answer:

#M_f=1.2xx10^(-5)M#

Explanation:

When a solution is diluted, the number of mole of particles in the solution does not change.

The relationship between the number of mole #n# and the molarity #M# is the following:

#M=n/V=>n=MxxV#

where, #V# is the volume of the solution.

If we consider that initially the volume and the molarity are:

#M_i=3.0xx10^(-5)M#

#V_i=40 mL#

What would be the final molarity #M_f=?# when the final volume is #V_f=100mL#?

since the number of mole does not change, we can write:

#M_ixxV_i=M_fxxV_f#

#=>M_f=(M_ixxV_i)/(V_f)=(3.0xx10^(-5)Mxx40cancel(mL))/(100cancel(mL))=1.2xx10^(-5)M#

Here is a video that discusses the solution preparation and dilution:
Lab Demonstration | Solution Preparation & Dilution.