(a) Calculate the [Fe3+ of each standard solution (samples 1-5 in your lab proce

Question

(a) Calculate the [Fe3+ of each standard solution (samples 1-5 in your lab procedure) taking into account the initial dilution (4mL/100mL) of the 0.0025 M stock solution and the subsequent dilution in each test tube. Remember moles remain the same in any dilution, and molarity volume -moles. (b) Show all work for one sample calculation as a component of this pre-lab assignment. (c) Record the values in your table for test tubes 1-5, as you will need these concentrations as you run the experiment. Table 1. composition of standard solutions for the determination of E-I diluted Fe(NO3)3 (mL) 0.0 M KSCN0.1 M HNO3total volume test tube (mL) 5.0 5.0 5.0 5.0 5.0 4.0 (mL) 10 (mL) 5.0 4.0 3.0 2.0 0 2.0 3.0 4.0 5.0 2 4

Explanation / Answer

The concentration of Fe+3 solution after dilution will be

M1V1 = M2V2

M1 = 0.0025

V1 = 4mL

V2 = 100

M2 =?

M2 = Concnetration after dilution = 0.0025 X 4/ 100= 0.0001 M

a) if we are taking 1mL of above solution then moles = 0.0001 X 1 millimoles

Final total volume = 10mL

so concentration of Fe+3 = 0.0001 / 10 = 0.00001 M

b) if we are taking 2mL of above solution then moles = 0.0001 X 2 millimoles

Final total volume = 10mL

so concentration of Fe+3 = 0.0002 / 10 = 0.00002 M

c) if we are taking 3mL of above solution then moles = 0.0001 X 3millimoles

Final total volume = 10mL

so concentration of Fe+3 = 0.0003/ 10 = 0.00003 M

d) if we are taking 4mL of above solution then moles = 0.0001 X 4 millimoles

Final total volume = 10mL

so concentration of Fe+3 = 0.0004/ 10 = 0.00004M

e) if we are taking 5mL of above solution then moles = 0.0001 X 5millimoles

Final total volume = 10mL

so concentration of Fe+3 = 0.0005 / 10 = 0.00005 M

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