What is the pH at the equivalence point for the titration of 0.24 M solutions of
ID: 540184 • Letter: W
Question
What is the pH at the equivalence point for the titration of 0.24 M solutions of the following acids and bases... C5H11N (piperidine) and HNO3. NaHSO3 and NaOH. Ba(OH)2 and HBr. What is the pH at the equivalence point for the titration of 0.24 M solutions of the following acids and bases... C5H11N (piperidine) and HNO3. NaHSO3 and NaOH. Ba(OH)2 and HBr. What is the pH at the equivalence point for the titration of 0.24 M solutions of the following acids and bases... C5H11N (piperidine) and HNO3. NaHSO3 and NaOH. Ba(OH)2 and HBr.Explanation / Answer
pH of salt formed = 7-1/2(pkb+logC)
pkb of PIPERIDINE = 2.8
C = concentration of salt = 0.24
pH = 7-1/2(2.8+log0.24)
= 5.91
At equivalence point ,
pka2 of H2SO3 = 7.18
pH of salt = 7+1/2(pka2+logC)
= 7+1/2(7.18+log0.24)
= 10.28
Ba(OH)2 (aq) + HBr(aq) ----> BaBr2(aq) + H2O(l)
here both acid,bases are strong.so that pH= 7 at equivalence point.
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