What is the pH of a .01100 M solution of NH3

Chemistry
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What is the pH of a .01100 M solution of NH3?

setup please

May 19th, 2015

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Use NH3 + HOH --> (NH4+) + (OH-)

Kb = 1.8 x 10^-5    (given in a textbook - rate constant)

Kb = (NH4+)(OH-)/(NH3) = (x^2)/0.01100

1.8 x 10^-5 = (x^2)/0.01100

x = 0.000445 = OH

p(OH) = -log(OH)

p(OH) = -log(0.000445)

p(OH) = 3.35

pH + pOH = 14

pH + 3.35 = 14

pH = 10.7 (approximately)



May 20th, 2015

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