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    Chemistry: molar solubility, hydroxide concentrations, ph level

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    The Ksp of La(IO3)3 is 1.0×10-11. Using activities, what is the molar solubility of La(IO3)3 in a 0.050 M solution of NaNO3?

    Using activities, calculate the hydroxide concentration in a saturated solution of iron (II) hydroxide in 0.010 M magnesium nitrate. The Ksp for Fe(OH)2 is 7.9×10-16, assume that Mg(NO3)2 dissociates completely

    What is the pH of a 3.6×10-8 M solution of HNO3.

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    Solution Preview

    The Ksp of La(IO3)3 is 1.0×10-11. Using activities, what is the molar solubility of La(IO3)3 in a 0.050 M solution of NaNO3?

    The dissociation equation for La(IO3)3 is:

    La(IO3)3  La3+ + 3IO3-
    Initial concn ------- 0 0
    Change s 3s
    Equilibrium concn s 3s

    Note = s is the concentration of saturated solution, hence the molar solubility

    Ksp = a La3+(a IO3-)3 where a = activity =  [X]

     = activity coefficient

    [X] = concentration of species

    Ksp =  La3+[ La3+]( IO3-[ IO3-])3
    Ksp =  La3+ (s) (IO3-)3 (3s)3
    Ksp = 1 x 10-11 = 27s4 (La3+) (IO3-)3

    To solve for activity coefficient ():

    • calculate ionic strength (µ)
    µ = ½  miZi2

    NaNO3  Na+ + NO3-
    0.05 M 0.05 0.05

    µ = ½ [(0.05)(1)2 + ...

    Solution Summary

    Molar solubility, hydroxide concentrations and ph levels in chemistry are examined. The activities are given.

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