What is the final concentration of an iron III nitrate solution that is prepared

Question

What is the final concentration of an iron III nitrate solution that is prepared by diluting 4.75 mL of 0.00300 M Fe(NO_3)_3 solution to a final volume of 10.00mL with deionized water (D.I. H_2O)? When you make your four solutions for this experiment, you will be adding 10.00 mL of methyl red stock solution, then other chemicals as listed on p.26, and finally diluting to 100.0 mL. The stock solution of methyl red contains 0.0800 g of the methyl red compound per liter of solution. The structural formula of methyl red is shown on p.23. The molecular formula is C_15 N_3 O_2 H_15. a. What is the molarity of the stock solution provided for this experiment? b. What is the molarity of methyl red in the 4 solutions that you prepare as described above?

Explanation / Answer

(1)

Dilution factor, D = Final volume/Initial volume = 10/4.75 = 2.105

So, final conc = Initial conc/D = 0.003/2.105 = 0.001425 M

(2)

MW of methyl red = 269.3 g

(a)

So, conc of stock = 0.08 g/L = (0.08/269.3) moles/L = 0.00029 M

(b)

Dilution factor, D = Final volume/Initial volume = 100/10 = 10

So, final conc = Initial conc/D = 0.00029/10 = 0.000029 M

Hope this helps !

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