CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon


Question

100 mL of a 0.5 M CH3COONa(aq) is titrated against a 0.5 M HCl(aq). Calculate the pH of the solution initially i.e. when no HCl has been added.
Given: pKa(CH3COOH)=4.74
 
  1. 6.58
  2. 8.24
  3. 7.96
  4. 9.22


Solution

The correct option is D 9.22
When only 100 mL of a 0.5 M CH3COONa(aq) is present. It will show simple salt hydrolysis. 
The formula to calculate the pH of a salt of strong base and weak acid is :
pH=12(pKw+pKa+log C)pH=12(14+4.74+log0.5)pH=12(18.741+log 5)pH=12(18.44)pH=9.22

flag
 Suggest corrections
thumbs-up
 
0 Upvotes


Similar questions
QuestionImage
QuestionImage
View More...


People also searched for
QuestionImage
QuestionImage
View More...



footer-image