Buffers are the solution that resists the change in pH. 1.39 ml of 5.90 M sodium hydroxide must be added to raise the pH to 5.75.
<h3>What is Henderson–Hasselbalch equation?</h3>
Henderson–Hasselbalch equation is used to determine the pH of the buffer by the equilibrium concentration of the acid and the conjugate base.
Moles of acetic acid are calculated as:
Moles of sodium acetate are calculated as:
The total number of moles is = 0.02352
Now, using the Henderson–Hasselbalch equation:
Given,
pH = 5.75
pKa = 4.74
Substituting values in the above equation:
Solving further:
Moles of acetate is calculated as:
0.02352 moles - 0.002093 moles = 0.021427 moles
Initial moles of acetate were 0.0132, added moles of acetate by the addition of the sodium hydroxide resulted in, 0.021427 - 0.0132 = 0.00822 moles of sodium hydroxide.
Volume is calculated as:
Therefore, 1.39 mL of 5.90M of sodium hydroxide is added.
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