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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

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