Calculate ph of buffer solution acetic acid and sodium acetate

Asked by admin @ in Chemistry viewed by 318 People

Calculate the ph of 0.375 l of a 0.18 m acetic acid-0.29 m sodium acetate buffer after the addition of 0.0090 mol of koh. assume that the volume remains constant.

Answered by admin @


To calculate the pH of this solution, we use the
Henderson-Hasselbalch equation: 


pH = pKa + log ([A-]/[HA])


Where,


[A-] = Molarity of the conjugate base =
CH3COO- = 0.29 M
[HA] = Molarity of the weak acid  = CH3COOH = 0.18 M


pKa = dissociation constant of the weak acid =
4.75


When KOH is added to the buffer, the chemical
reaction is:


CH3COOH + KOH = CH3COO-K+ + H2O


Therefore when 0.0090 mol KOH is added, 0.0090
mol acid is neutralized, and 0.0090 mol CH3COO- is produced.


[CH3COO-] = [0.0090 mol + 0.375 L (0.29 mol/L) ]
/ 0.375 L = 0.314 M


[CH3COOH] = [-0.0090 mol + 0.375 L (0.18 mol/L) ]
/ 0.375 L = 0.156 M


Going back to Henderson-Hasselbalch
equation:


pH = 4.75 + log (0.314 / 0.156)


pH = 5.054


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