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

$$M_{base}=0.173M$$

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:

$$n_{acid}=M_{base}V_{base}$$

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

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

Best regards!