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1- Calculate the equilibrium concentration for H+, HSO4- and SO4^2- , given a .150M H2SO4 solution. the Ka for HSO4- is 1.20*10^-2


    The first ionization is 100%; therefore,
    ..........H2SO4 ==> H^+ + HSO4^-

    The second H is weak.
    ............HSO4^- ==> H^+ + SO4^2-

    k2 = 0.012 = (H^+)(SO4^2-)/(HSO4^-)
    Substitute the E line of the second ICE chart and solve for x, then
    total (H^+) = 0.150+x
    (SO4^2-) = x
    (HSO4^-) = 0.150-x
    Of course (H2SO4) = 0

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