Hydroxylamine is a weak molecular base with kb = 6.6 x 10-9. what is the ph of a 0.0500 m solution of hydroxylamine?

Question

Chemistry

Carly Hayden

28 February, 14:55

Hydroxylamine is a weak molecular base with kb = 6.6 x 10-9. what is the ph of a 0.0500 m solution of hydroxylamine?

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Answers (1)

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Blake Small · Answer 1

Answer is: pH of hydroxylamine solution is 9,23.

Kb (NH₂OH) = 1,8·10⁻⁵.

c ₀ (NH₂OH) = 0,0500 M = 0,05 mol/L.

c (NH ₂⁺) = c (OH⁻) = x.

c (NH₂OH) = 0,05 mol/L - x.

Kb = c (NH ₂⁺) · c (OH⁻) / c (NH₂OH).

0,0000000066 = x² / (0,05 mol/L - x).

solve quadratic equation: x = c (OH⁻) = 0,000018 mol/L.

pOH = - log (0,000018 mol/L) = 4,74.

pH = 14 - 4,74 = 9,23.