Question

In: Chemistry

A reaction is carried out by combining 65.00 mL of a 0.108 M sample of (NH4)3PO4...

A reaction is carried out by combining 65.00 mL of a 0.108 M sample of (NH4)3PO4 and 48.00 mL of a 0.230 M Fe9NO3)2 solution. The net ionic equation is :

3Fe^2+(aq) + 2PO4^3-(aq) ---> Fe3(PO4)2(s) balanced

1a) What is the mass of iron(II) phosphate (MM= 357.49 g/mol) produced in the reaction?

1b) What are the concentrations of the reacting ions (Fe^2+(aq) and PO4^3+(aq)) at the end of the reaction (assuming no change in volume)?

Solutions

Expert Solution

3 Fe(NO3)2 + 2 (NH4)3PO4 = Fe3(PO4)2(s) + 6 (NH4)NO3 ................i

Complete Ionic Reaction is written as

3Fe2+ + 6NO3- + 6NH4+ + 2PO43- = Fe3(PO4)2(s) + 6NO3- + 6NH4+...................ii

And Net Ionic Equation is

3Fe2+(aq) + 2PO43-(aq) ---> Fe3(PO4)2(s).................iii

Now given that

[(NH4)3PO4] = 0.108 and V= 65 ml

Moles of (NH4)3PO4 = 0.108 mol/L*0.065 L = 0.00702 mol

Fe(NO3)2 =0.230 M , V= 48 mol

Moles of Fe(NO3)2 = 0.230 * 0.048 =0.011 mol

3Fe2+ + 6NO3- + 6NH4+ + 2PO43- = Fe3(PO4)2(s) + 6NO3- + 6NH4+

Now complete ionic reaction shows that

3 Fe(NO3)2 + 2 (NH4)3PO4 = Fe3(PO4)2(s) + 6 (NH4)NO3

From reaction 2: 3 mol of Fe(NO3)2 gives 2 mol Fe2+ and 6 mol NO3-

So for 0.011 mol Fe(NO3)2 , Fe2+ = 0.0073 mol and NO3- = 0.022 mol

From reaction 2: 2 mol of (NH4)3PO4, gives 6 mol NH4+ and 2 mol PO43-

So, for 0.00702 mol of (NH4)3PO4 0.0210 mol NH4+ and 0.00702 mol PO43-

Now

Net reaction

3Fe^2+(aq) + 2PO4^3-(aq) ---> Fe3(PO4)2(s)

From this reaction: 3 mol Fe2+ will react with 2 mol PO43- to form 1 mol Fe3(PO4)2

We calcuated that initial concentrations of Fe2+ = 0.0073 mol and PO43- = 0.00702 mol

Here limiting reactant is Fe2+

So, 0.073 mol of Fe2+ will react with 0.0049 mol of PO43-to form 0.00243 mol Fe3(PO4)2

From reaction 2:

a) Total 0.00243 mol Fe3(PO4)2 will form in this reaction.

Mass of Fe3(PO4)2 produced = 0.00243 mol*357.49 g/mol = 0.869 g

b) Final concentrations of Fe2+(aq) & PO43- are

Fe2+ is limiting so, Fe2+ concentration= 0

Final moles of PO43- = Initial-consumed = 0.00702-0.0049 = 0.00212 mol

Total volume is 48+65 m= 113 ml= 0.113 L

Final concentration of Fe2+= 0

Final concentration of PO43- = 0.00212/0.113 = 0.0188 M


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