The half‑equivalence point of a titration occurs half way to the equivalence point, where half of...

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The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to

A volume of 500.0 mL of 0.120 M NaOH is added to 565 mL of 0.250 M weak acid (K4 = 1.63 x 10-5). What is the pH of the result

The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyze has reacted to form its conjugate, and the other half still remains unreacted.

If 0.4400.440 moles of a monoprotic weak acid (?a=7.2×10−5)(Ka=7.2×10−5) is titrated with NaOH,NaOH, what is the pH of the solution at the half‑equivalence point?

pH=pH=

2)

A volume of 500.0 mL500.0 mL of 0.120 M0.120 M NaOHNaOH is added to 565 mL565 mL of 0.250 M0.250 M weak acid (?a=1.63×10−5).(Ka=1.63×10−5). What is the pHpH of the resulting buffer?

HA(aq)+OH−(aq)⟶H2O(l)+A−(aq)HA(aq)+OH−(aq)⟶H2O(l)+A−(aq)

pH=

2)

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