This question concerns the titration of 10.0 mL of 0.0400 M NaOH with 0.0200 M H

Question

This question concerns the titration of 10.0 mL of 0.0400 M NaOH with 0.0200 M HCl. Neglect activity coefficients and assume 25 °C.

Write the net ionic equation for the titration reaction. What is the numerical value of its equilibrium constant (call it Ktitr)? Is it safe to claim that this reaction “goes to completion”? What is the pH at the equivalence point? Ignoring ionic strength and temperature effects, why should you expect the same equivalence point pH for any strong acid/strong base titration?

Please show all work! Thank You!

Explanation / Answer

The net reaction:

NaOH + HCl ----> NaCl + H2O

The net ionic reaction taking place is:

H+ + OH- ---> H2O

At 270C, the equilibrium constant for this reaction has the value 10-14 M2

Since this reaction is between a strong acid and a strong base, the reaction should theoretically go to completion. But ideally speaking no reaction ever goes to completion.

The pH for this neutralization reaction is 7.

For any stong acid/base titartion, the net ionic reaction taking place is the same as for the above case.

Thus, essentially every such titration produces the same net pH value of 7 at the equivalence point.

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