I was given the following problem:
what is the normality of a solution containing 6 grams of H2SO4 in a 200ml solution? my teacher obtained a normality of 39normals while I took into account that I had two hydrogen free and obtained a result of 0.6 N, who's right?

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  1. .6 is correct ... due to H⁺ activity

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  2. Did you make a typo and you meant to type in that the teacher obtained 0.30 N?
    Technically, you can't say. Both could be right but I disagree with Scott as to why that is so. You must know the equation involved. For example, if you titrate one(1) H then
    mL x N x milliequivalent weight = grams.
    200 x N x 0.098 = 6g and N = 0.31 which rounds to 0.3 N to 1 sig fig. and the equation is
    NaOH + H2SO4 ==> NaHSO4 + H2O

    if the equation is
    2NaOH + H2SO4 ==> Na2SO4 + 2H2O then
    200 x N x 0.049 = 6 and N = 0.61 which rounds to 0.6 to 1 s.f.
    The equivalent weight of H2SO4 is 98 when 1 H is used but it is 98/2 = 40 when both H atoms are used.

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