Calculate the pH of the following aqueous solution: 0.37 M NH4Cl (pKb for NH3 = 4.74)
Calculate the pH of the following aqueous solution: 0.37 M NH4Cl (pKb for NH3 = 4.74)
Ammonium chloride is a salt of Weak base(NH3) and strong acid (HCl)
In aqueous medium the hydrolysis of NH4Cl is given as,
NH4Cl + H2O < --------- > NH4+ + Cl-
NH4+ + HO-H < ------- > NH4OH + H+
Because of this the aqueous solution of NH4Cl is acidic.
For aqueous solution of weak base-strong acid pH is given as,
pH = 7 – ½(pKb)- ½ (log[salt])
We have, pKb = 4.74, [salt] =[NH4Cl] = 0.37 M
So, pH = 7 – ½(4.74)- ½ log[0.37]
pH = 7 – 2.37 – ½ (0.432)
pH = 4.63 – 0.216
pH = 4.414.
pH of aq. 0.37 M NH4Cl solution is 4.414.
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