Chemistry

posted by .

FeSCN2+ -> Fe3+ + SCN-
Solution is initially dark red. If some Ag+ is added to form AgSCN. what happens to position of equilibrium? what happens ot the color?

  • Chemistry -

    AgSCN is a white ppt. Adding Ag^+ will ppt AgSCN and that removes the SCN^- from solution which will shift the equilibrium to the right. If enough Ag^+ is added, all of the FeSCN^+2 complex (red) will be used up and you will be left with a white ppt of AgSCN + iron(III) ions.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    The correct interpretation of the equation below is: Fe3+(aq) + SCN–(aq) --> and <-- FeSCN2+(aq) A. A heterogeneous equilibrium exists because of the charged ions. B. At equilibrium, the rate of the forward reaction equals …
  2. chemistry

    The correct interpretation of the equation below is: Fe3+(aq) + SCN–(aq) --> FeSCN2+(aq) A. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. B. The equilibrium constant is Kc = [Fe3+][SCN–][FeSCN2+] …
  3. chemistry

    The correct interpretation of the equation below is:?
  4. CHEMISTRY HELP! ICE TABLES?

    At a certain temperature, K = 9.1 10-4 for the following reaction. FeSCN2+(aq)= Fe3+(aq) + SCN -(aq) Calculate the concentrations of Fe3+, SCN -, and FeSCN2+ in a solution that is initially 4.0 M FeSCN2+. OKAY SO i started by doing …
  5. chemistry

    In a certain trial, the initial concentrations of Fe3+ and SCN- are both 1.00x10^-3 M and the initial concentration of FeSCN2+ is zero. Suppose that after the reation reaches equilibrium, the concentration of FeSCN2+ was found to be …
  6. Chemistry

    A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration of FeSCN2+ ([FeSCN2+]std) for this standard solution is assumed to be M. What permits this …
  7. Chemistry

    A reaction mixture of 4.0 mL of 0.002 M SCN- and 5.0 mL of 0.002 M Fe3+ is diluted to 10.0 mL with 0.1 M HNO3 to form the blood-red FeNCS2+ complex. The equilibrium molar concentration of the FeNCS2+ determined from a standardization …
  8. Chemistry

    A student mixes 5.0 mL of 0.00200 M Fe(NO3)3 with 5.0 mL 0.00200 KSCN. She finds that the concentration of FeSCN2+ in the equilibrium mixture is 0.000125 M. Follow these steps to determine the corresponding experimental value of Kc …
  9. chemistry

    A reaction mixture of 4.0 mL of 0.002 M SCN- and 5.0 mL of 0.002 M Fe3+ is diluted to 10.0 mL with 0.1 M HNO3 to form the blood-red FeNCS2+ complex. The equilibrium molar concentration of the FeNCS2+ determined from a standardization …
  10. Chemistry

    I am having trouble getting the right answer for this question please help. Calculate Kc for the FeSCN2+ formation equilibrium [FeSCN2+] = 3.49x10^-5 M [Fe3+] = 4.39x10^-4 M [SCN-] = 1.93x10^-4 Kc = [FeSCN2+] / ([Fe3+]-[FeSCN2+]) * …

More Similar Questions