For 550.0 mL of a buffer solution that is 0.150 M in CH3CH2NH2 and 0.140 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.010 mol of HCl.
this is a "basic" buffer, since there is weak base + conjugate acid:
CH3CH2NH2 + H2O <--> CH3CH2NH3+ + OH-
and
CH3CH2NH3Cl --> CH3CH2NH3+ + Cl-
so there is weak base and conjguate acid
now...
pOH = pKb + log(CH3CH2NH3+ / CH3CH2NH2 )
pKB for ethylamine = 3.19
so
initially:
mmol of base = MV = 550*0.15 = 82.5 mmol of base
mmol of conjugate = MV = 550*0.140 = 77 mmol of conjugate
calculate initial pH:
pOH = pKb + log(CH3CH2NH3+ / CH3CH2NH2 )
pOH = 3.19 + log(77 /82.5) = 3.16
pH = 14-3.16 = 10.84
after:
addition of 0.01 mol of HCl = 0.01*1000 = 10 mmol of H+
mmol of base = 82.5 -10 = 72.5 mmol
mmol of conjguate acid = 77 + 10 = 87
so
pOH = pKb + log(CH3CH2NH3+ / CH3CH2NH2 )
pOH = 3.19 + log(87/72.5) = 3.26918
pH = 14-3.26918= 10.730
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