Which of the following solutions would have [Fe3+]=0.020M?
0.40 L of 0.050 M Fe(NO3)3
0.80 L of 0.020 M Fe2(NO3)3
0.50 L of 0.040 M Fe2(C2O4)4
0.50 L of 0.040 M FeC6H5O7
explain your answer
To determine the concentration of [Fe3+] in each solution, we can use the balanced equation for the dissociation of the compound.
1. The balanced equation for the dissociation of Fe(NO3)3 is:
Fe(NO3)3(s) → Fe3+(aq) + 3 NO3-(aq)
Therefore, the concentration of [Fe3+] will be equal to the concentration of Fe(NO3)3.
[Fe3+] = 0.050 M
2. The balanced equation for the dissociation of Fe2(NO3)3 is:
Fe2(NO3)3(s) → 2 Fe3+(aq) + 6 NO3-(aq)
Therefore, the concentration of [Fe3+] will be twice the concentration of Fe2(NO3)3.
[Fe3+] = 2 * 0.020 M = 0.040 M
3. The balanced equation for the dissociation of Fe2(C2O4)4 is:
Fe2(C2O4)4(s) → 2 Fe3+(aq) + 4 C2O42-(aq)
Therefore, the concentration of [Fe3+] will be twice the concentration of Fe2(C2O4)4.
[Fe3+] = 2 * 0.040 M = 0.080 M
4. The balanced equation for the dissociation of FeC6H5O7 is:
FeC6H5O7(s) → Fe3+(aq) + C6H5O7^2-(aq)
Therefore, the concentration of [Fe3+] will be equal to the concentration of FeC6H5O7.
[Fe3+] = 0.040 M
Among the given solutions, the one with [Fe3+] = 0.020 M is the 0.40 L of 0.050 M Fe(NO3)3 solution.