Question

9.48 What is the pH of an aqueous solution consisting of
0.070 M formic acid (HCOOH) and 0.070 M sodium
formate (HCOONa)?​

Answer 1

Answer:

Explanation:

Use the Henderson-Hasselbalch equation.

pH = pKa + log (base)/(acid) ,

pH = ? ,

pKa = look up ,

(base) = 0.07 ,

(acid) = 0.07,

pKa = 7.6 for HCOOH ,

so pH= 7.6 + log [.07]/[.07} ,

pH = 7.6.

Hope it helps.