According to Henderson–Hasselbalch Equation,
pH = pKa + log [Acetate] / [Acetic Acid]
As, pKa of Acetic Acid = 1.76
So, pH = 1.76 + log [Acetate] / [Acetic Acid]
4.70 = 1.76 + log [Acetate] / [Acetic Acid]
4.70 - 1.76 = log [Acetate] / [Acetic Acid]
-0.04 = log [Acetate] / [Acetic Acid]
Taking Antilog on both sides,
[Acetate] / [Acetic Acid] = 0.912
