What volume (in mL) of 1.0 M HCl is required to prepare 1000 mL of pH 7.76 buffer using triethanolamine that is 0.020 M in both triethanolamine and triethanolammonium ion?
[base] =triethanolamine
[salt] = triethanolammonium ion
moles of both salt and base = 0.02 x 1000 / 1000 = 0.02
[salt ] + [base] = 0.02-------------------->1
pH = 7.76
pOH = 6.24
HCl + base ----------------> salt + H2O
pOH = pKb + log [salt / base]
6.24 = 6.2 + log [salt / base]
[salt / base] = 1.096
[salt] = 1.096 [base] ------------------> 2
[base] + 1.096 [base] = 0.02
[base] = 0.0095
[salt] = 0.01 moles
salt moles = HCl moles
HCl moles = 0.01
HCl molarity = moles / volume
1.0 = 0.01 / volume
volume = 0.01 L
volume of HCl = 10ml
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