Lab Question. Calculate the concentration of each standard in terms of ppm iron.
ID: 949047 • Letter: L
Question
Lab Question. Calculate the concentration of each standard in terms of ppm iron. FW= 392.14 g/mol. Please show your work.First prepare standard solution from a standard Fe stock of 0.13 M. Make 100x dilution (1 mL of stock into 100 mL of water)
Then, using a pipet deliver the following volumes of your Fe standard diluted solution into 10 mL volumetric flasks: 0 mL, 150 micro liters, 300 microliters, 450 mL, and 600mL Lab Question. Calculate the concentration of each standard in terms of ppm iron. FW= 392.14 g/mol. Please show your work.
First prepare standard solution from a standard Fe stock of 0.13 M. Make 100x dilution (1 mL of stock into 100 mL of water)
Then, using a pipet deliver the following volumes of your Fe standard diluted solution into 10 mL volumetric flasks: 0 mL, 150 micro liters, 300 microliters, 450 mL, and 600mL
First prepare standard solution from a standard Fe stock of 0.13 M. Make 100x dilution (1 mL of stock into 100 mL of water)
Then, using a pipet deliver the following volumes of your Fe standard diluted solution into 10 mL volumetric flasks: 0 mL, 150 micro liters, 300 microliters, 450 mL, and 600mL
Explanation / Answer
When we make 100x dilution, the new concentration concantration can be calculated as
0.13M x V = M x 101V
=> M = 0.13 / 101 = 1.29x10-3 M = 1.29x10-3 mol/L
Molecular mass of the iron compound = 392.14 g/mol
Hence concentration of the standard diluted solution = 1.29x10-3 mol x 392.14 g/mol / L = 0.505 g/L
= 0.505 g x (1000 mg / g) / L = 505 mg/L = 505 ppm (answer)
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