The pH of a 1.0 L solution of 0.10 M lactic acid is 4.34. What is the new pH of the solution if 40 mL of 1.0 M HCl is added? The pKa of lactic acid is 3.86.
The pH of a 1.0 L solution of 0.10 M lactic acid is 4.34. What is the new pH of the solution if 40 mL of 1.0 M HCl is added? The pKa of lactic acid is 3.86.
Assume that moles of acid x
Then moles of base = 0.10 –X
the Henderson-AHasselbalch equation is
pH = pKa + log(c_base/c_acid)
the original pH is
4.34 = 3.86 + log(X/0.10-X)
log(X/0.10-X) = 0.48
X/0.10-X= 10^0.48
X/0.10-X=3.02
X = 0.302 -3.02X
4.02 X= 0.302
X= 0.075
Moles of acid =0.075
Moles of base = 0.025
moles H+ added = 40 x 10^-3 L x 1.0M
=0.04
new moles lactic acid = 0.0075 + 0.04
0.0475
Molarity = 0.0475 /1.040
= 0.0456
moles lactate = 0.0025 - 0.04
= -0.0375
Molarity = -0.0375/1.040
= - 0.036
pH = 3.86 + log 0.0456/ (-0.036)
pH = 3.86 + (-0.103)
= 3.757
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