2mL of a 10M solution of Compound A is taken and 48mL added. 1mL of this solution is then taken and dried to dryness before being re-dissolved in 0.1mL. What is the concentration of the 0.1mL solution?

0.04

Well, if Compound A were a person, it would definitely be feeling diluted right now!

Let's break it down. You started with a 2 mL solution of Compound A that was 10 M in concentration. Then, you added 48 mL to it. So now you have a total volume of 2 mL + 48 mL, which is 50 mL.

To find the new concentration, we need to consider how much Compound A is now present in the 50 mL solution. Since the total volume is now 50 mL, and you started with 2 mL of a 10 M solution, you initially had 2 mL * 10 M = 20 moles of Compound A.

However, when you added 48 mL to the initial 2 mL, the number of moles of Compound A remained the same! So now you still have 20 moles of Compound A, but in a larger volume of 50 mL.

Now, we can use this information to find the concentration of the 0.1 mL solution. Since you started with 20 moles of Compound A in a 50 mL solution, you can set up a proportion:

20 moles / 50 mL = x moles / 0.1 mL

Simplifying this gives us:

x moles = (20 moles / 50 mL) * 0.1 mL

x moles = 0.04 moles

Therefore, the concentration of the 0.1 mL solution is 0.04 moles / 0.1 mL, which is equal to 0.4 M.

So, the concentration of the 0.1 mL solution is 0.4 M. Just like a good cup of coffee, it's strong in a small package!

To find the concentration of the 0.1 mL solution, we can use the concept of dilution.

Let's break down the information given step-by-step:

1. Initially, 2 mL of a 10 M solution of Compound A is taken.
2. Then, 48 mL is added to the 2 mL solution. This results in a total volume of 2 mL + 48 mL = 50 mL.
3. 1 mL of this 50 mL solution is then taken.
4. The 1 mL solution is dried to dryness, which means all the solvent is removed.
5. The dried residue is re-dissolved in 0.1 mL.

Now, let's calculate the concentration of the 0.1 mL solution:

Since 1 mL of the 50 mL solution was taken, this means that the 0.1 mL solution is 1/10th of the 1 mL. Therefore:

Concentration of the 0.1 mL solution = concentration of the 1 mL solution / 10.

The concentration of the 1 mL solution can be calculated using the molarity formula:

Molarity (M) = moles of solute / volume of solution in liters.

Since the volume is given in mL in this case, we need to convert it to liters by dividing by 1000.

Moles of solute = Molarity x Volume (in liters)

Given that the initial solution is 10 M and the volume is 1 mL, we have:

Moles of solute = 10 M x 1 mL / 1000 = 0.01 moles.

Now, we can calculate the concentration of the 0.1 mL solution:

Concentration of the 0.1 mL solution = 0.01 moles / 10 = 0.001 moles / mL.

Therefore, the concentration of the 0.1 mL solution is 0.001 moles/mL.

To find the concentration of the 0.1 mL solution, we need to understand the dilution process and use the given information step by step.

Step 1: Calculate the amount of Compound A in the initial 2 mL solution.
The initial 2 mL solution has a concentration of 10 M, which means there are 10 moles of Compound A in 1 liter of the solution. Since we have 2 mL of the solution, we need to convert it to liters:
2 mL = 2/1000 L = 0.002 L.
So, the initial 2 mL solution contains:
10 M x 0.002 L = 0.02 moles of Compound A.

Step 2: Calculate the amount of Compound A after dilution.
48 mL is added to the initial 2 mL solution. So we have a total volume of 2 mL + 48 mL = 50 mL.
To get the final concentration, we can use the formula: M1V1 = M2V2, where:
- M1 is the initial concentration (0.02 moles/L)
- V1 is the initial volume (2 mL or 0.002 L)
- M2 is the final concentration (unknown)
- V2 is the final volume (50 mL or 0.05 L).
We can rearrange the formula to solve for M2:
M2 = (M1 x V1) / V2
Plugging in the values:
M2 = (0.02 moles/L x 0.002 L) / 0.05 L
M2 = 0.0008 moles/0.05 L
M2 = 0.016 moles/L.

Step 3: Calculate the concentration of the 0.1 mL solution.
1 mL of the 50 mL solution (from step 2) is taken and dried to dryness, then re-dissolved in 0.1 mL.
Since the solution was dried to dryness, the amount of Compound A remains the same, but the volume changes.
We have the final concentration from step 2 (0.016 moles/L) and the final volume is now 0.1 mL or 0.0001 L.
Using the formula: M1V1 = M2V2:
(0.016 moles/L) x V1 = (unknown concentration) x 0.0001 L
The unknown concentration = (0.016 moles/L x V1) / 0.0001 L
Again, rearranging the formula:
Unknown concentration = (0.016 moles/L x V1) / 0.0001 L

To find the unknown concentration, we need the volume V1. If V1 is not given, it is not possible to determine the concentration of the 0.1 mL solution.