In: Chemistry
56.0 mL of 2.50 M Fe(NO3)2 is combined with 25.0 mL of 0.0525 M Na2CO3.
Ksp of FeCO3 is 2.1 × 10-11.
What mass of FeCO3(s) will be produced? in grams
What is the [Fe2+] in the solution final solution? in M
What is the [CO32-] in the solution final solution? in M
Given that 56 mL of 2.5 M Fe(NO3)2
= 56 mL x 2.5 mole / 1000 mL
= 0.14 moles
Given that 25 mL of 0.0525 M Na2CO3
= 25 mL x 0.0525 mole / 1000 mL
= 0.0013125 moles
Consider the equation
Fe(NO3)2 + Na2CO3 FeCO3 + 2 NaNO3
Initial moles 0.14 0.0013125 0 0
after reaction (0.14 - 0.0013125) 0 0.0013125 0.002625
= 0.1387
mass of FeCO3 produced = 0.0013125 x molecular mass of FeCO3
= 0.0013125 x 115.85 = 0.152 g
Total volume after reaction = 56 + 25 = 81 mL = 0.081 L
Therefore concentration of Fe(NO3)2 after reaction = 0.1387 mole / 0.081 L
= 1.712 M
Therefore concentration of Fe2+ in the resultant solution = 1.712 M
This is due to the excess of Fe(NO3)2
Given that the solubility product of FeCO3 is 2.1 x 10-11
[Fe] [CO3] = 2.1 x 10-11
Consider the equation FeCO3 Fe2+ + CO32-
[x] [ x]
Where [x] is the concentration of Fe2+ CO32- and in the solution
But already we have the concentration of Fe2+ due to the excess of Fe(NO3)2 = 1.712 M
Therefore the total conc of Fe2+ = [Fe2+] = [1.712 + x]
and [CO32-] = [x]
Ksp = 2.1 x 10-11 = [1.712 + x] * [x]
= 1.712x [since x is small compared to 1.712 it is neglected in [1.712 + x]
therefore x = 2.1 x 10-11 / 1.712 = 1.23 x 10-11 M
Thus
The mass of FeCO3 produced = 0.152 g
[Fe2+] in the final solution = 1.712 M
[CO32-] in the final solution = 1.23 x 10-11 M