Hydrofluoric acid, HF, is a weak acid with an acid-dissociation constant (Ka) of 6.3 ✕ 10−4. If 0.023 L of 0.17 M HF is titrated with 0.16 M NaOH, a strong base, determine the pH at the equivalence point. (The ion-product constant of water isKw = 1.01 ✕ 10−14 at 25°C.)
at equivalence point : millimoles of acid = millimoles of base
0.023 x 0.17 = 0.16 x V
V = 0.024 L
total volume = 0.023 + 0.024 = 0.047 L
at equivalence point only salt is remains
salt concentration = 0.023 x 0.17 / total volume
= 0.083 M
pKa = -log Ka
pKa = 3.20
pH = 7 + 1/2 [pKa + logC]\
pH = 7 + 1/2 [3.20 + log 0.083]
pH = 8.06
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