Determine the equilibrium concentration of the base HS− given that Kb=1.0×10−7 and the equilibrium concentrations of...
Determine the equilibrium concentration of the base HS− given that Kb=1.0×10−7 and the equilibrium concentrations of OH− and H2S are 6.0×10−4 M, and 4.4×10−7 M respectively.
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![Кь = х 101 K, я к = K = 14 15 » к = K = 1xis : xo7 Сон-] = 6. охоч - сн+) = (хоч = 1.661 хо м 6. охоч [ths I = 4.4x10M H₂S](http://img.homeworklib.com/questions/95d8cb40-cfc0-11eb-8e6c-31865a8066c0.png?x-oss-process=image/resize,w_560)
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Determine the equilibrium concentration of the base HS− given
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Determine the equilibrium concentration of the base NH3 given that pKb=4.76 and the equilibrium concentrations of OH− and NH+4 are 6.5×10−5 M, and 0.42 M respectively. Report your answer with two significant figures.
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For a 1.0 M solution of H2S at equilibrium, which of the following statements are correct?...
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The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
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