What mass of sodium hydroxide must be added to 75.0 mL of 0.205 M acetic acid in order to create a buffer with a pH of 4.74? acetic acid Ka=1.8x10^-5
(Answer is 0.31g how do we arrive there?)
Ans. Step 1: Calculate pKa of acid
pKa = -log Ka = -log (1.8 x 10-5) = 4.74
Step 2: Calculate relative concertation of weak acid and its conjugate base
Using Henderson- Hasselbalch equation –
pH = pKa + log ([A-] / [AH]) - equation 1
where, A- = conjugate base (CH3COONa or simply CH3COO-)
AH = Weak acid (CH3COOH)
Putting the values in equation 1-
4.74 = 4.74 + log ([A-] / [AH])
Or, 4.74 – 74.74 = log ([A-] / 0.100)
Or, [A-] / [AH] = antilog 0 = 1
Or, [A-] / [AH] = 1
Hence, [A-] = [AH] = 1
That is, at pH 4.74 both the acid and its conjugate base are at same concentration.
Now,
Let [A-] = [AH] = X
So, total concentration of [A-] and [AH] at equilibrium is-
[A-] + [AH] = 2X
Given, total initial [AH] = 0.205 M
It is the initial [AH] that dissociates to form equilibrium [A-]. The remaining un-dissociated initial [AH] (i.e. total initial [AH] – dissociated [AH] = [AH] at equilibrium)] is equal to [AH at equilibrium.
So,
([A-] + [AH]) at equilibrium = Total initial [AH]
Or, 2X = 0.205 M
Hence, X = 0.205 M/ 2 = 0.1025 M
That is, at equilibrium, [A-] = [CH3COONa] = 0.1025 M
Step 3: Calculating required amount of NaOH.
Balanced reaction: CH3COOH + NaOH ---------> CH3COONa + H3O+
Stoichiometry: 1 mol NaOH reacts with 1 mol CH3COOH to form 1 mol CH3COONa.
Moles of CH3COONa at equilibrium = Molarity x Volume of solution in liters
= 0.1025 M x 0.075 L ; [1 L = 103 mL]
= (0.1025 mol/ L) x 0.075 L ; [1 M = 1 mol/ L]’
= 0.0076875 mol
Note the stoichiometry of balanced reaction, 1 mol NAOH produces 1 mol CH3COONa.
So,
Moles of NaOH required = 0.0076875 mol = Moles of CH3COONa at equilibrium
Mass of NaOH required = Moles x Molar mass
= 0.0076875 mol x (40.00 g/mol)
= 0.3075 g
= 0.31 g
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