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18 November, 14:18

How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 14.0 L of a solution that has a pH of 2.12?

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  1. 18 November, 15:47
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    W=0.360

    p=1.18g/mL

    pH=2.12

    v=14.0 L

    M (HCl) = 36.46 g/mol

    v₀-?

    1) pH=-lg[H⁺]

    [H⁺]=c (HCl) = 10^ (-pH)

    n (HCl) = v[H⁺]=v*10^ (-pH)

    2) n (HCl) = m (HCl) / M (HCl) = wv₀p/M (HCl)

    3) v*10^ (-pH) = wv₀p/M (HCl)

    v₀=v*10^ (-pH) M (HCl) / (wp)

    v₀=14.0*10^ (2.12) * 36.46 / (0.360*1.18) = 9.115 mL

    Approximately 9.1 mL of concentrated solution required.
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