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    Solubility, Concentration and Precipitation Problems

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    At 25 degrees C, the value of Ksp for PbCl2(s) is 1.6x10^-5 and the value of Ksp for AgCl(s) is 1.8x10^-10.
    1) If 60.0mL of 0.0400 M NaCl (aq) is added to 60.0mL of 0.0300M Pb(NO3)2(aq) will a precipitate form? Assume that the volumes are additive. Show calculations to support your answer.

    2) Calculate the equilibrium value of Pb+2 (aq) in 1.00L of saturated PbCl2 solution to which 0.250 moles of NaCl(s) has been added. Assume that no volume change occurs.

    3) If 0.100 M NaCl(aq) is added slowly to a beaker containing both 0.120M AgNO3(aq) and 0.150 M Pb(NO3)2 (aq) at 25 degrees C, which will precipitate first, AgCl (s) or PbCl2(s)? Show calculations to support your answer.

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    https://brainmass.com/chemistry/stoichiometry/solubility-concentration-precipitation-problems-174607

    Solution Preview

    At 25 degrees C, the value of Ksp for PbCl2(s) is 1.6x10^-5 and the value of Ksp for AgCl(s) is 1.8x10^-10.
    1) If 60.0mL of 0.0400 M NaCl (aq) is added to 60.0mL of 0.0300M Pb(NO3)2(aq) will a precipitate form? Assume that the volumes are additive. Show calculations to support your answer.

    The reaction to form the precipitate will be:
    Pb2+ + 2 Cl- ---> PbCl2(s)
    The Ksp expression is: Ksp = [Pb2+][Cl-]2
    Now, find [Cl-] and [Pb2+] to see if precipitation will ...

    Solution Summary

    Concentration and Precipitation Problems are explained.

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