Chemistry

posted by .

Equal volumes of 0.240 M AgNO3 and 0.140 M ZnCl2 solution are mixed. Calculate the quilibrium concentrations of Ag+, and Zn2+.

  • Chemistry -

    ZnCl2(aq) + 2AgNO3(aq) ==> Zn(NO3)2(aq) + 2AgCl(s)
    I would assume a convenient volume of each, say 100 mL, then
    (ZnCl2) = (Zn^+2) = 100mL x 0.140M = 14 mmoles/200 mL = 0.070M Zn ion.
    (Cl^-) = 2 x 14 = 28 mmoles Cl^-

    The Ag^+ is trickier because AgCl is insoluble AND you have some of the Cl^-, which is in excess, acting as a common ion which decreases the solubility of AgCl.
    AgCl(s) ==> Ag^+ + Cl^-
    Ksp = (Ag^+)(Cl^-) = 1.82E-10
    (Ag^+) = Ksp/(Cl^-).
    You know Ksp. (Cl^-) is done this way. AgCl formed is 24 mmoles which uses up all of the Ag in the AgCl and 24 of the 28 Cl^- in the ZnCl2. So there are 4 mmoles Cl^- in excess and (Cl^-) = mmoles/mL = 4 mmoles/200 mL = ??
    Then substitute that into the (Ag^+) = Ksp/(Cl^-) and solve for Ag^+. I don't know if this was a trick question your prof gave you or if your prof wanted you to be on your toes and recognize that a ppt was formed and there was a common ion present.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    We are doing a lab that requires finding the molarity of an unknown AgNO3 solution after reacting NaCl + AgNO3 --> NaNO3 and AgCl and collecting/massing the precipitate. We will be using 10.00 mL of an NaCl solution and 10.00 mL …
  2. Chemistry

    What is the concentration of NO3- ions when equal volumes of 0.1M AgNO3 and 0.1M NaCl are mixed together?
  3. chemistry

    this is a lab i am working on and this is what is says: Solution A is mixed with water to produce solutions of varying concentration. These altered concentrations of solution A is added to a set amount of solution B and the reaction …
  4. chemistry

    What percentage of the Ba2+ in solution is precipitated as BaCO3(s) if equal volumes of 2.4*10^-3 M Na2CO3(s) and 1.1*10^-3M BaCl2(aq) are mixed
  5. Chemistry

    At room temperature, 80.0 ml of 0.125 M AgNO3(aq) and 20.0 ml of 0.500 M Fe(NO3)2(aq) are mixed together, generating the following equilibrium system Ag+ (aq) + Fe2+(aq) Ag(s) + Fe3+(aq). At equilibrium, the concentration of Fe3+ is …
  6. chemistry

    A 7.00 g sample of KCl is dissolved in 81.0 mL of water. The resulting solution is then added to 28.0 mL of a 0.790 M CaCl2(aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the …
  7. Chemistry

    Silver ion reacts with excess CN− to form a colorless complex ion, Ag(CN)−2, which has a formation constant Kf=3.0×1020. Calculate the concentration of Ag+ in a solution prepared by mixing equal volumes of 2.3×10−3M …
  8. chemistry

    Equal volumes of 0.220 M weak base (Kb=4.0x10^-9) and 0.220 M HCl are mixed. Calculate the pH of the resulting solution
  9. chemistry

    Calculate the concentrations of all ions after 50.0 mL of a 0.100 M AgNO3 solution is mixed with 100.0 mL of a 1.00 M Na2SO4 solution.For Ag2SO4 Ksp = 1.2 x 10-5 Do I first do MiVi=MfVf and then using the two concentrations I use ksp …
  10. Chemistry

    the pH of a solution is 10 and other is 12 when equal volumes of these low are mixed the pH of the resulting solution is?

More Similar Questions