CH3NH3Cl is a salt weak base CH3NH2 and strong acid HCl.
CH3NH3Cl + H2O CH3NH2 + HCl
CH3NH3+ + H2O CH3NH2 + H+
ICE table is
CH3NH3- | CH3NH2 | H+ | |
I | C | - | - |
C | -C | +C | +C |
E | C - C | C | C |
Dissociation constant is Kh , degree of dissociation is
Or, - log[H+] = - log Kw + logKb - logC
pH = pKw - pKb - logC
Or, pH = 7 - (3.36 ) - log(0.10)
Or, pH = 7 - 1.68 + 0.5
Or, pH = 5.82
[ Kb of CH3NH2 = 4.36×10-4, or pKb = 3.36]
4.
NH4CN is salt of weak acid and weak base
Hence,
pH = 7 + (pKa - pKb)
Ka of HCN = 4.9×10-10, pKb = - logKb = - log(4.9×10-10) = 9.3
Kb of NH3 = 1.8×10-5 . Or, pKa = 4.75
Hence, pH = 7 + ( 9.30 - 4.75) = 7 + 2.275 = 9.275
use a table of ka and kb to determine pH of the 0.10 M CH3NH3Cl d....
Determine the pH of a 0.10 M CH3NH3Cl solution. (Kb (CH3NH2) = 4.4 x 10-4) 2.18 11.82 5.82 8.17 3.36
Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. 1.61 8.75 5.25 12.39
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