Respuesta :
Answer:
The equilibrium concentration of FeSCN²⁺ is 0.0002 M
Explanation:
Given data:
9 mL of 0.2 M of Fe(NO)₃
1 mL of 0.002 M of KSCN
Question: What is the equilibrium concentration of FeSCN²⁺
Calculate the initial millimoles of Fe(NO₃)₃:
[tex]n_{Fe(NO3)3} =0.2\frac{mmoles}{mL} *9mL=1.8mmol[/tex]
Initial millimoles of KSCN:
[tex]n_{KSCN} =0.002\frac{mmoles}{mL} *1=0.002mmoles[/tex]
Total volume of solution:
Vtotal = 1 + 9 = 10 mL
Initial concentration of Fe(NO₃)₃:
[tex][Fe(NO3)3]=\frac{1.8}{10} =0.18M[/tex]
Initial concentration of KSCN:
[tex][KSCN]=\frac{0.002}{10} =0.0002M[/tex]
The reaction:
SCN⁻ + Fe³⁺ → FeSCN²⁺
I 0.0002 0.18 0
C -0.0002 -0.0002 0.0002
E 0 0.1798 0.0002
As you see the equilibrium concentration of FeSCN²⁺ is 0.0002 M
