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A 18.4 mL sample of a monoprotic weak acid, HX, was titrated to the equivalence point...

A 18.4 mL sample of a monoprotic weak acid, HX, was titrated to the equivalence point with 25.7 mL of 0.308 M NaOH. What is the pH at the equivalence point for this titration (HX has Ka = 4.66

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Answer #1

First calculate the concentration of the acid HX.

Now calculate the concentration of the conjugate base of the acid.

Write the equilibrium reaction for the hydrolysis of the conjugate base.

Prepare an ICE table.
Initial concentration (M) 0.1795 0 0
Equilibrium concentration (M) x x

Write the equilibrium constant expression.

Substitute values in the above expression.

Since the value of the equilibrium constant is very small,

Write the modified equilibrium constant expression.

Calculate the pOH of the solution.

Calculate the pH of the solution.

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