Chemistry

posted by .

Ca(IO3)2(s) ⇌ Ca^(2+)(aq) + 2IO3^(-)(aq)

First, you poured 30 mL of 0.100 M Ca^(2+) solution over a 2.000 g sample of solid Ca(IO3)2 and allowed the mixture to sit for 30 minutes. Some of the solid dissolved, causing the calcium ion concentration to increase by a certain quantity and the iodate concentration to increase by two times that certain quantity. Next, you isolate the filtrate through gravity filtration. What do you expect the iodate concentration to be in the filtered solution? How would the iodate concentration differ if only a 0.500 g sample of the solid was used? What if the solvent was water instead?

  • Chemistry -

    This is a solubility product problem with Ca^+2 as a common ion.
    Ca(IO3)2 ==> Ca^+2 + 2IO3^-

    Ksp = (Ca^+2)(IO3^-)^2
    If we call the solubility of Ca(IO3)2 = X, then (Ca^+) = X in the equilibrated solution and (IO3^-) = 2X.
    Now plug those values into Ksp.
    (0.1 + X)(2X)^2 = Ksp.
    Solve for X and multiply by 2 to find IO3^-.
    Next, no difference if 0.5 g sample of Ca(IO3)2 used. Finally, your last question doesn't make any sense? The solvent IS water isn't it? instead of what? It dissolves in water.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Easy chem question... me=braindead, help please?

    It's been so long I forget which ones are which. My balanced equation is Sr(NO3)2 + 2KIO3 --> Sr(IO3)2 + 2KNO3. It wants the total ionic and the net ionic Thanks ^^ (not just looking for answer, want explanation too please, just …
  2. CHEMISTRY

    Wondering If I did this correctly so far 50.0 ml of a 0.0500 M solution of lead (II) nitrate is mixed with 40.0 ml of a 0.200 M solution of sodium iodate at 25°C. Calculate the Pb2+ and IO3- concentrations when the mixture comes to …
  3. chemistry

    OKOK I know that I have posted this question but I just don't understand the last part. 50.0 ml of a 0.0500 M solution of lead (II) nitrate is mixed with 40.0 ml of a 0.200 M solution of sodium iodate at 25°C. Calculate the Pb2+ and …
  4. Chemistry

    Given these chemical reactions: Ca^(2+)(aq) + 2IO3^(-)(aq) → Ca(IO3)2(s) Ca(NO3)2·4H2O(s) → Ca^(2+)(aq) + 2NO3^(-)(aq) + 4H2O(l) KIO3(s) → K^(+)(aq) + IO3(-)(aq) Calculate the masses of Ca(NO3)2·4H2O(s) and KIO3(s) …
  5. chemistry (quatatative analysis)

    How many grams of Ba(IO3)2 can be dissolved in 500 mL of a 0.100 M KIO3 solution at 25 oC?
  6. Chemistry

    A solution containing Pb2+ and a solution containing IO3- are poured together and quickly mixed. After mixing, the solution contains 0.0030 M Pb2+ and 0.040 M IO3-. Immediately Pb(IO3)2(s), which has Ksp=2.510-13, begins to precipitate. …
  7. Chem

    At 298 K, Pb(IO3)2(s) ↔ Pb2+(aq) + 2IO3-(aq) Ksp = 2.6x 10-13 Pb2+(aq) + 2e- → Pb(s) Eo = (-0.126) V. Find the standard potential of the half-reaction: Pb(IO3)2(s) + 2e- ↔ Pb(s) + 2IO3-(aq) Eo = ?
  8. Chemistry

    Calculate the concentration of IO3– in a 9.23 mM Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 × 10-13. Assume that Pb(IO3)2 is a negligible source of Pb2 compared to Pb(NO3)2.
  9. Chemistry

    Hello, I would greatly appreciate some help with the following problem, as I'm not sure how to proceed. I'm trying to find solubility (Ksp) of Cu(IO3)2 from titration experiment. The following equations were provided: Cu(IO3)2 --> …
  10. chem

    Calculate the concentration of IO3– in a 4.73 mM Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 × 10-13. Assume that Pb(IO3)2 is a negligible source of Pb2 compared to Pb(NO3)2.

More Similar Questions