Calculate pH of a buffer prepared by adding 10 mL of 0.10 M acetic acid to 20 mL of 0.1 M sodium acetate. [pKa (CH3COOH) = 4.74 ]
![How should the acid dissociation constant pKa be measured? | Automatic Potentiometric Titrators | Faq | Kyoto Electronics Manufacturing Co.,Ltd.("KEM") How should the acid dissociation constant pKa be measured? | Automatic Potentiometric Titrators | Faq | Kyoto Electronics Manufacturing Co.,Ltd.("KEM")](https://www.kem.kyoto/en/wp-content/uploads/sites/2/2021/03/%E3%82%B9%E3%83%A9%E3%82%A4%E3%83%891-e1616636994970.png)
How should the acid dissociation constant pKa be measured? | Automatic Potentiometric Titrators | Faq | Kyoto Electronics Manufacturing Co.,Ltd.("KEM")
![SOLVED: Question #16: In buffer calculations, we used the Henderson-Hasselbalch equation. [A-] pH = pKa + logâ‚ â‚€ [THA] Suppose you are using a weak monobasic acid, HA, with a pKa of SOLVED: Question #16: In buffer calculations, we used the Henderson-Hasselbalch equation. [A-] pH = pKa + logâ‚ â‚€ [THA] Suppose you are using a weak monobasic acid, HA, with a pKa of](https://cdn.numerade.com/ask_previews/3d97130d-3610-4ac7-8aee-a2500b0f71f3_large.jpg)
SOLVED: Question #16: In buffer calculations, we used the Henderson-Hasselbalch equation. [A-] pH = pKa + logâ‚ â‚€ [THA] Suppose you are using a weak monobasic acid, HA, with a pKa of
![SOLVED: Calculate Ka and pKa of the acid using pH and molarity. Moles of unknown acid = 0.001215. Molar mass of acid = 172.84. Molarity = 0.243 mol/L. pH = 2.06. Ka = [ SOLVED: Calculate Ka and pKa of the acid using pH and molarity. Moles of unknown acid = 0.001215. Molar mass of acid = 172.84. Molarity = 0.243 mol/L. pH = 2.06. Ka = [](https://cdn.numerade.com/ask_previews/f6745ba3-6b77-4e7a-9de2-7d980958d194_large.jpg)