What is the pH of a solution that is 0.456 M in diethylamine (CH3CH2)2NH and 0.547 M in diethylamine chloride (CH3CH2)2N...

Question

Question

What is the pH of a solution that is 0.456 M in diethylamine (CH₃CH₂)₂NH and 0.547 M in diethylamine chloride (CH₃CH₂)₂NH₂Cl?

The K_b for diethylamine is 6.9 x 10^-4.

Answer 1

Answer #1

pKb = - logKb

pKb = - log( 6.9 ×10^-4) = 3.16

pKa = 14 - pK_b

pK_a of (CH3CH2)2NH2⁺ = 14 - 3.16 = 10.84

Henderson - Hasselbalch equation which gives pH of a buffer solution

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

pH = 10.84 + log ( 0.456M/0.547M)

pH = 10.84 - 0.08

pH = 10.76

Answer 2

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