Calculate the volume of 0.320-M NaOH solution needed to completely neutralize 74.0 mL of a 0.230-M solution of the monoprotic acid HBr. mL N

Question

Calculate the volume of 0.320-M NaOH solution needed to completely neutralize 74.0 mL of a 0.230-M solution of the monoprotic acid HBr. mL NaOH.

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Verity 3 years 2021-07-17T12:05:01+00:00 1 Answers 11 views 0

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  1. kimcuc
    0
    2021-07-17T12:06:29+00:00
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    Answer:

    53.2 mL

    Explanation:

    As this problem deals with the neutralization of a strong monoprotic acid and a strong base, we can solve it by using the following formula:

    • Ca * Va = Cb * Vb

    Where in this case:

    • Ca = 0.230 M
    • Va = 74.0 mL
    • Cb = 0.320 M
    • Vb = ?

    We input the data:

    • 0.230 M * 74.0 mL = 0.320 M * Vb

    And solve for Vb:

    • Vb = 53.2 mL

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