CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon


Question

Find the pH of 1 L of a buffer solution containing 0.01 M NH4Cl and 0.05 M NH4OH at 25C
The base dissociation constant for NH4OH is 1.8×105
Take log(1.8)=0.26
  1. 11.56
  2. 12.56
  3. 9.96
  4. 10.36


Solution

The correct option is C 9.96
This is a basic buffer formed by a weak base (NH4OH) and its salt (NH4Cl) with strong acid (HCl)
pKb=log(Kb)pKb=log(1.8×105)pKb=(50.26)=4.74
pOH=pKb+log[salt][base]pOH=pKb+log([NH4Cl][NH4OH])pOH=4.74+log(0.010.05)pOH=4.74+log(0.2)=(4.740.7)pOH=4.04pH+pOH=14pH=14pOH=144.04=9.96

flag
 Suggest corrections
thumbs-up
 
0 Upvotes


Similar questions
View More


People also searched for
View More



footer-image