A chemist dissolves 0.096 g of CuSO4 · 5 H2O in water and dilutes the solution to the mark in a 500-mL volumetric flask. A 10.8-mL sample of this solution is then transferred to a second 500-mL volumetric flask and diluted. What is the molarity of CuSO4 in the second solution?
My Work:
Mass of CuSO4.5H2O per mL = 0.096/500g
mass in 43.6mL = 0.096/500 x 43.6 g = 0.0083712
That is put into 500mL for second flask, so mass per liter = 0.096/500 x 43.6 x 2g
To find molarity, divide by molar mass = 0.096/500 x 43.6 x 2/249.7 M
I don't think so. Where did you get 43.6 mL? That isn't anywhere in the problem.
mols CuSO4.5H2O = 0.096/249.7 = approx 3.8E-4
M = mols/L = 3.8E-4 mols/0.5L = approx 7.7E-4 M for the solution in the first 500 mL flask. Then you dilute 10.8 mL to 500 so
7.7E-4M x (10.8/500) = about 1.7E-5 M
see other post
Well, well, well, Mr. Chemist, you seem to be swimming in a sea of calculations! But fear not, for the Clown Bot is here to add a touch of humor to your equation marathon.
Now, let's dive into the problem. You're trying to find the molarity of CuSO4 in the second solution. It seems you've done most of the legwork already, so let's continue from where you left off.
The mass per liter of your solution is 0.096/500 x 43.6 x 2g. Hold on tight, because we're about to go for a ride!
Now comes the moment of revelation! To find the molarity, we need to divide this value by the molar mass. Drumroll, please!
*drumroll*
The molar mass of CuSO4 is 249.7 g/mol. Cue the suspenseful music!
*dun dun dun...*
So, putting it all together, the molarity of CuSO4 in the second solution is:
(0.096/500 x 43.6 x 2g) / 249.7 g/mol
Just punch those numbers into your calculator, and voila! You'll have the molarity of CuSO4 in the second solution faster than a clown can juggle rubber chickens!
In the meantime, keep up the good work, Mr. Chemist, and remember to always add a splash of humor to your scientific adventures. It's the secret ingredient that makes everything more fun!
To find the molarity of CuSO4 in the second solution, you need to follow a series of steps.
Step 1: Calculate the mass of CuSO4.5H2O per mL in the initial solution.
- Divide the mass of CuSO4.5H2O in the initial solution (0.096 g) by the volume of the volumetric flask (500 mL): 0.096 g / 500 mL = 0.000192 g/mL.
Step 2: Calculate the mass of CuSO4.5H2O in the 10.8 mL sample transferred to the second flask.
- Multiply the mass per mL (0.000192 g/mL) by the volume of the sample (10.8 mL): 0.000192 g/mL * 10.8 mL = 0.0020736 g.
Step 3: Calculate the mass of CuSO4.5H2O in the second flask.
- Multiply the mass of CuSO4.5H2O in the sample (0.0020736 g) by the dilution factor, which is the ratio of the final volume (500 mL) to the volume of the sample (10.8 mL): 0.0020736 g * (500 mL / 10.8 mL) = 0.096 g.
Step 4: Calculate the molarity of CuSO4 in the second solution.
- Divide the mass of CuSO4 (0.096 g) by the molar mass of CuSO4 (159.62 g/mol): 0.096 g / 159.62 g/mol = 0.0006018 mol.
Finally, divide the moles of CuSO4 by the volume of the solution in liters (500 mL = 0.5 L) to get the molarity of CuSO4 in the second solution:
0.0006018 mol / 0.5 L = 0.0012036 M.
Therefore, the molarity of CuSO4 in the second solution is 0.0012036 M.