In a titration of hydrobromic acid (HBr) against sodium hydroxide (NaOH), 22.20 mL of 0.150 M NaOH is required to neutralize 36.60 mL of HBr

Question

In a titration of hydrobromic acid (HBr) against sodium hydroxide (NaOH), 22.20 mL of 0.150 M NaOH is required to neutralize 36.60 mL of HBr. Calculate the molarity of the HBr. M1V1=M2V2

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King 6 months 2021-07-26T08:15:58+00:00 1 Answers 8 views 0

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    2021-07-26T08:17:33+00:00

    Answer:

    [HBr] = 0.0910 M

    Explanation:

    NaOH → Strong base

    HBr → Strong acid.

    This is a titration that involves a strong acid and a strong base, so the recaction is about acid base equilibrium.

    Formula for titration in the equivalence point is:

    mmoles of acid = mmoles of base

    M . Volume of acid = M . volume of base

    We replace data:

    M . 36.60 mL = 0.150 M . 22.20 mL

    M = (0.150 M . 22.20 mL) / 36.60 mL

    M = 0.0910 mol/L

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Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )