Chemistry

posted by .

If very small concentrations of NaCl and AgNO3 are mixed, no precipitate forms. However, if large concentrations are mixed, a white precipitate forms.
Can someone tell me a method for testing the hypothesis that "insoluble" salts would dissolve to some extent in water and are slightly soluble. If the Ksp is low,the solid is not soluble and if high, it is soluble and if it the product of the ion concentration does the exceed the Ksp value, no precipate would form.So that's the hypothesis.So, can someone give me a experiment to test this hypothesis.

  • Chemistry -

    What about using an electrochemical set up to show that AgCl is slightly soluble. You would measure the (Ag^+) in the cell.

  • Chemistry -

    One difficulty you will have at very low amounts of NaCl and AgNO3, the precipate is so scarce you cannot see it. So my question is, in your test for a precipate, what is your test?

  • Chemistry -

    thanks for your suggestion. but maybe is it possible to use the titration method to determine whether or not the precipate would for form, for example, adding the large concentration of AgNO3 and NaCl which would cause the precipitate to form and then use those values obtained from the titration to work out the Ksp value.However, if the ionic concentration is equal to or more than the Ksp then the precipitate would form. And, for the small concentration, i would add the small volumes of NaCl and AgNO3, doing the same method and calculating the Ksp, where if the ionic concentration is less than the Ksp, then no precipitate would form.Would that method be alright or not effective in finding out if precipate would form or not?

    And the method you mentioned about using electrochemical set-up to show that AgCl is slightly soluble,can you explain in detail what the experiment would consist of? Thanks!!

  • Chemistry -

    With regard to the electrochemical set up, I was proposing that you prepare AgCl in sufficient quantity, add it to a fresh sample of water, let it form a saturated solution, filter, then measure the (Ag^+) in the filtrate. That would show that you have Ag^+ in solution. That would show that "insoluble" salts do, in fact, dissolve to a small extent. That would also get around Bob Pursley's legitimate concern that very small amounts of AgCl ppts are not visible to the naked eye. The electrochemical method is one way in which Ksp values are determined in the first place.
    With regard to your proposal, I don't think it gets around the concern Bob Pursley has about "seeing" the very small amounts of AgCl formed.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chem

    if 50 mL of .012M barium chloride are mixed with 25 mL of 1.0 x 10^-6M sulfuric acid, will a precipitate form?
  2. chemistry

    An AgNO3 solution (44 mL/0.44 M) has been mixed with an NaCl solution (83 mL/1.35x 10^-2 M) a)Determine the ion product of the precipitate(potential precipitate) b) Would a precipitate be created?
  3. Chemistry

    When sulfuric acid is added to magnesium nitrate, is the resulting product soluble or insoluble in water?
  4. Chemistry

    If I added sodium carbonate to magnesium nitrate, would it be insoluble & a precipitate forms?
  5. Chemistry

    I am very confused on this problem. Any help would be great: 50 g of silver nitrate is mixed with 50 g of hydrochloric acid in a water-based solution. A white precipitate forms (silver chloride.) The solution is filtered and the white …
  6. CHEM

    Will you please tell me if these are right?
  7. Chemistry

    If very small concentrations of NaCl and AgNO3 are mixed, no precipitate forms. However, if large concentrations are mixed, a white precipitate forms. Can someone tell me a method for testing the hypothesis that "insoluble" salts would …
  8. ap chemistry

    When 50.0 mL of a 0.010 M CuNO3 solution is mixed with 150.0 mL of a 0.010 M NaCl solution, a precipitate forms (Ksp = 1.9 x 10^-7). a) Determine all final ion concentrations b) Determine the mass of the precipitate formed. How do …
  9. Chem Help!

    Assume that a given solution caontains Ag+or Ba2+ or a mixture of both. A reasonable method for doing a qualitative analysis on this solution might be sketched out as followes (remember || means a precipitate forms and | means a solution …
  10. chemistry

    When calcium chloride and ammonium phosphate are mixed, an insoluble precipitate of calcium phosphate forms and falls out of solution. After careful analysis of the purified precipitate, 8.16 * 10^25 atoms of calcium are found in the …

More Similar Questions