If 0.8675 g of KHP requires 24.56 mL of an NaOH solution to reach the equivalence point in the titration, what is the concentration of

Question

If 0.8675 g of KHP requires 24.56 mL of an NaOH solution to reach the equivalence
point in the titration, what is the concentration of the NaOH?

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Kiệt Gia 1 year 2021-09-04T13:27:50+00:00 1 Answers 3 views 0

Answers ( )

  1. RobertKer
    0
    2021-09-04T13:29:08+00:00
    Reply

    Answer:

    [tex]M_{base}=0.173M[/tex]

    Explanation:

    Hello there!

    In this case, since the titration of acids like KHP with bases like NaOH are performed in a 1:1 mole ratio, it is possible for us to know that their moles are the same at the equivalence point, and the concentration, volume and moles are related as follows:

    [tex]n_{acid}=M_{base}V_{base}[/tex]

    Thus, by solving for the volume of the base as NaOH, we obtain:

    [tex]M_{base}=\frac{n_{acid}}{V_{base}} \\\\M_{base}=\frac{0.8675g*\frac{1mol}{204.22g} }{0.02456L} \\\\M_{base}=0.173M[/tex]

    Best regards!

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