Calculate the pH of 100.0 mL of a buffer that is 0.0500 M NH4Cl and 0.125 M NH3 before and after the addition of 1.00 mL of 5.40 M HNO3.
pH before =
pH after =
i) Befor addition
Henderson - Hasselbalch equation is
pOH = pKb + log([Conjucate acid ]/ [ Base] )
= 4.75 + log ( [ NH4+ ]/[NH3])
= 4.75 + log(0.0500M/0.125M)
= 4.75 - 0.40
= 4.35
pH + pOH = 14
pH = 14 - pOH
= 14 - 4.35
= 9.65
b) After addition
Initial mole of NH3 =(0.125mol/1000ml)×100ml = 0.0125mol
Initial mole of NH4+= (0.050mol/1000ml)×100ml =0.0050mol
Mole of HNO3 added = (5.40mol/1000ml)×1ml = 0.0054mol
HNO3 react with base NH3 to form NH4+
NH3 + HNO3 ------> NH4+ + NO3-
0.0054mol of HNO3 react with 0.0054mole of NH3 to form 0.0054 mole of NH4+
After addition
No of mole of NH3 = 0.0125 - 0.0054 = 0.0071
No of mole of NH4+ = 0.0050 + 0.0054 = 0.0104
Total volume = 101ml
[ NH3] = (0.0071mol/101ml)×1000ml = 0.0703M
[ NH4+ ] = ( 0.0104mol/101ml)×1000ml = 0.1030M
Applying Henderson equation
pOH = 4.75 + log(0.1030M/0.0703M)
= 4.75 + 0.17
= 4.92
pH = 14 - 4.92
= 9.08
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