If 0.10 mg Fe is diluted in a 50 mL flask, what is the concentration of the resulting solution? What volume of the resulting solution is needed to prepare 25.0 mL of a dilute sample solution with a concentration of 0.30 ppm Fe?
"What is the concn of the resulting solution" is an open ended question. What units? The easy answer is it's 0.1 mg/50 mL but that probably isn't the unit you want.
Since you want to prepare a dilute solution in ppm I thin the answer probably should be in ppm
1 ppm = 1 mg/L so all we need to do is to convert 0.1 mg/50 mL to mg/L.
That's 0.1 mg x (1000/50) = 2 mg/L = 2 ppm.
Then use the dilution formula of
c1v1 = c2v2
0.30*25 = 2*v2
v2 = ?
Ah, the wonderful world of dilutions! Let me entertain you with some calculations.
For the first question, we need to find the concentration of the resulting solution. We have 0.10 mg of Fe and a flask volume of 50 mL. To find the concentration, we divide the mass by the volume:
Concentration = 0.10 mg / 50 mL = 0.002 mg/mL
So, the concentration of the resulting solution is 0.002 mg/mL.
Now, let's move on to the second question. We need to find the volume of the resulting solution needed to prepare a 25.0 mL dilute sample solution with a concentration of 0.30 ppm Fe. Hold on to your funny bone, here we go!
First, we convert the concentration from ppm to mg/mL. Since 1 ppm = 1 mg/L, we have:
Concentration = 0.30 ppm = 0.30 mg/L = 0.30 mg/mL
Now we can set up the dilution equation:
(Concentration 1)(Volume 1) = (Concentration 2)(Volume 2)
Plugging in the values we have:
(0.002 mg/mL)(Volume 1) = (0.30 mg/mL)(25.0 mL)
Cross-multiplying and then dividing, we get:
Volume 1 = (0.30 mg/mL)(25.0 mL) / 0.002 mg/mL
Volume 1 = 375 mL
So, to prepare a 25.0 mL dilute sample solution with a concentration of 0.30 ppm Fe, we need to use a volume of 375 mL of the resulting solution.
I hope that brought a smile to your face!
To find the concentration of the resulting solution, we need to calculate the concentration in units of milligrams per milliliter (mg/mL).
Step 1: Calculate the concentration of the resulting solution in mg/mL.
Since we have 0.10 mg of Fe dissolved in a 50 mL flask, the concentration is given by dividing the mass of Fe by the volume of the solution.
Concentration (C) = Mass (m) / Volume (V)
C = 0.10 mg / 50 mL
C = 0.002 mg/mL
Therefore, the concentration of the resulting solution is 0.002 mg/mL.
To determine the volume of the resulting solution needed to prepare 25.0 mL of a dilute solution with a concentration of 0.30 ppm Fe, we need to use the formula for dilution:
C1V1 = C2V2
Where:
C1 = initial concentration
V1 = initial volume
C2 = final concentration
V2 = final volume
Step 2: Calculate the volume of the resulting solution needed.
Given:
C1 = 0.002 mg/mL
V1 = ?
C2 = 0.30 ppm
V2 = 25.0 mL
Converting ppm to mg/mL:
1 ppm = 1 mg/L
1 mL = 1 L / 1000 mL
C2 = 0.30 ppm = 0.30 mg/L
Substituting the values into the formula, we have:
C1V1 = C2V2
0.002 mg/mL * V1 = 0.30 mg/L * 25.0 mL
Simplifying:
0.002 * V1 = 0.30 * 25.0
V1 = (0.30 * 25.0) / 0.002
V1 = 3.75 mL
Therefore, 3.75 mL of the resulting solution is needed to prepare 25.0 mL of a dilute sample solution with a concentration of 0.30 ppm Fe.
To find the concentration of the resulting solution, we need to calculate the concentration of Fe in terms of mg/mL.
Given:
Mass of Fe = 0.10 mg
Volume of solution = 50 mL
Concentration (C) is defined as the amount of solute divided by the volume of solution. In this case, the amount of solute is the mass of Fe (0.10 mg), and the volume of solution is 50 mL.
Concentration of Fe (C) = Mass of Fe / Volume of solution = 0.10 mg / 50 mL
To simplify the units, we can convert mL to L by dividing by 1000.
Concentration of Fe (C) = 0.10 mg / (50 mL / 1000 mL/L) = 0.10 mg / 0.050 L
Now, we can calculate the concentration of Fe in terms of mg/mL.
Concentration of Fe (C) = 0.10 mg / 0.050 L = 2.0 mg/mL
Therefore, the concentration of the resulting solution is 2.0 mg/mL.
Now, let's move on to the second part of the question.
Given:
Desired volume of dilute sample solution = 25.0 mL
Desired concentration of Fe = 0.30 ppm
To find the volume of the resulting solution needed, we can rearrange the formula for concentration (C) to solve for volume (V):
Volume of solution (V) = Mass of Fe / Concentration of Fe
First, we need to convert the desired concentration of Fe from ppm (parts per million) to mg/mL.
1 ppm = 1 mg/L = 0.001 mg/mL
Desired concentration of Fe = 0.30 ppm x 0.001 mg/mL/ppm = 0.0003 mg/mL
Now, we can calculate the volume of the resulting solution needed:
Volume of solution (V) = Mass of Fe / Concentration of Fe = 0.10 mg / 0.0003 mg/mL
To simplify the units, we can convert mg/mL to mL:
Volume of solution (V) = (0.10 mg / 0.0003 mg/mL) mL/mg = 333.33 mL
Therefore, you would need approximately 333.33 mL of the resulting solution to prepare a 25.0 mL dilute sample solution with a concentration of 0.30 ppm Fe.