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The pH of a solution obtained by mixing 5 mL of 0.1 M NH₄OH solution with 250 mL of 0.1 M NH₄Cl solution is _____ 10⁻² . (Nearest integer) Given: pK_b(NH₄OH) = 4.74 2 = 0.30 3 = 0.48 5 = 0.70

Correct answer

0

Step-by-step solution

The given mixture forms a basic buffer solution. Millimoles of base NH₄OH = 5 0.1 = 0.5 mmol Millimoles of salt NH₄Cl = 250 0.1 = 25 mmol Using the Henderson-Hasselbalch equation for a basic buffer: pOH = pK_b + ( [ Salt ] [ Base ] ) pOH = 4.74 + ( 25 0.5 ) pOH = 4.74 + (50) We know that (50) = (5 10) = 5 + 10 = 0.70 + 1 = 1.70 pOH = 4.74 + 1.70 = 6.44 The pH of the solution is given by: pH = 14 - pOH pH = 14 - 6.44 = 7.56 pH = 756 10⁻² Answer: 756

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