Chemistry

posted by .

A solution contains 0.133 g of dissolved Lead. How many moles of soduim chloride must be added to the solution to completly precipitate all of the disolved lead? What mass of sodium chloride must be added?

  • Chemistry -

    A solved example. Just follow the steps.
    http://www.jiskha.com/science/chemistry/stoichiometry.html

  • Chemistry -

    a solution contains 0.133 g of dissolved lead. How many moles of sodium chloride must be added to the solution to completely precipitate all of the dissolved lead? what mass of sodium chloride must be added?

  • Chemistry -

    Ok so first of all equation:
    Pb2+ + 2Cl- = PbCl
    Then we do some stoich
    so we find the mole of the lead n=m/M
    n=.133/207.2
    n=6.4x10^-4mol
    Now by using the mole ratio
    for every Lead solution ion there need to be 2 Sodium solution (sodium chloride) ions
    therefore double the amount in mol
    12.8x10^-4mol
    or
    1.28x10^-3mol

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    a precipitate is expected when an aqueous solution of potassium iodide is added to an aqueous solution of: sodium sulfate iron(II) chloride calcium perchlorate barium hydroxide lead nitrate
  2. chemistry

    A solution contains 0.245 of dissolved lead (lead ion or Pb2+.) How many moles of sodium chloride must be added to the solution to completely precipitate all of the dissolved lead?
  3. Chemistry

    A solution contains an unknown mass of dissolved silver ions. When potassium chloride is added to the solution, a white precipitate forms. The precipitate is filtered and dried and then found to have a mass of 245 mg. What mass of …
  4. Chemistry

    A solution contains 0.133 g of dissolved Lead. How many moles of sodium chloride must be added to the solution to completely precipitate all of the disolved lead?
  5. Chemistry

    7 grams of chloride was dissolved in water. 20 ml of lead(II)nitrate was used to completely precipitate all chloride (assume atomic mass of 35g/mol). What is the molarity of the Lead(II) Nitrate solution.
  6. Chemistry

    7 grams of chloride was dissolved in water. 20 ml of lead(II)nitrate was used to completely precipitate all chloride (assume atomic mass of 35g/mol). What is the molarity of the Lead(II) Nitrate solution.
  7. chemistry

    What concentration of the lead ion, Pb^{2+} , must be exceeded to precipitate PbCl2 from a solution that is 1.00 x 10^{-2} M in the chloride ion, Cl^- ?
  8. Chemistry

    A 10.00 gram solid sample consisting of a mixture of sodium chloride and potassium sulfate is dissolved in 100.0 mL of water is combined with another 200.0 mL solution that contains excess aqueous lead(II) nitrate. Upon mixing the …
  9. science

    In an experiment to determine the solubility of lead chloride (PbCl2), 5.6g of (NH4)2SO4 was added to a 250ml solution containing an unknown amount of dissolved lead chloride (PbCl2) resulting in the formation of Lead sulfate precipitate. …
  10. Chemistry

    80.0 ml of 1.50 M lead (IV) acetate is added to a 65.5 ml solution of 1.25 potassium chloride. 5.84 grams precipitate are collected. what is the percent yield?

More Similar Questions