I am hoping to receive help getting started with this problem, possibly some steps in the correct direction.

Here is the question: 5.0mLs of a 6.0M solution of HCl was transferred to a 1000ml volumetric flask and diluted to volume w/ water. 50mLs of this solution was then transferred to a 100mL flask and diluted to Volume with water. What is the molarity of the 2nd diluted solution?

Sorry, the second post was sent by mistake. No shouting intended! :)

Can some one check to see if I did this correct:

6M= moles of solute/.005 L solution

.03=moles solute

M of2nd solu=.03 m solute/.05L solution

M=.6

After the second dilution:

M of2nd solu=.03 m solute/.10L solution

Why .10L

I based on this, unless I mis-read it.

50mLs of this solution was then transferred to a 100mL flask and diluted to Volume with water...

To solve this problem, we can use the concept of dilution. Dilution is the process of reducing the concentration of a solution by adding more solvent (usually water). The key concept to understand here is that the number of moles of solute in the original solution remains constant despite dilution.

Here are the steps to solve the problem:

Step 1: Calculate the number of moles of HCl in the original 5.0 mL of 6.0 M solution.
- To do this, we can use the formula: moles = concentration (M) x volume (L).
- Convert the volume of the solution from mL to L by dividing it by 1000 since there are 1000 mL in 1 L.
- So, moles = 6.0 M x (5.0 mL / 1000 mL) = 0.03 moles

Step 2: Calculate the concentration of the first diluted solution in the 1000 mL volumetric flask.
- Since the original solution was diluted to volume with water, the number of moles of HCl remains the same, but the volume changes.
- To calculate the concentration, we can use the formula: concentration (M) = moles / volume (L).
- Convert the volume from mL to L by dividing it by 1000.
- So, concentration = 0.03 moles / (1000 mL / 1000) = 0.03 M

Step 3: Calculate the number of moles of HCl in the 50 mL of the first diluted solution.
- We can use the same formula: moles = concentration (M) x volume (L).
- Convert the volume from mL to L by dividing it by 1000.
- So, moles = 0.03 M x (50 mL / 1000 mL) = 0.0015 moles

Step 4: Calculate the concentration of the second diluted solution in the 100 mL volumetric flask.
- Again, since the moles of HCl remain the same and the volume changes, we can use the formula: concentration (M) = moles / volume (L).
- Convert the volume from mL to L by dividing it by 1000.
- So, concentration = 0.0015 moles / (100 mL / 1000) = 0.015 M

Therefore, the molarity of the second diluted solution is 0.015 M.