Dianfeng Chemical
SUPPLEMENTS
HydrogenSulfideGasReactionWithExcessPotassiumHydroxideSolution
Reaction of hydrogen sulfide gas into excess potassium hydroxide solution
Hydrogen sulfide is also a gas with rotten egg odor. When this gas is slowly introduced into excess potassium hydroxide solution, the two chemically react.
Potassium hydroxide is a strong base, and the concentration of hydroxide ions ($OH ^ - $) in its solution is quite high. Hydrogen sulfide ($H_2S $) is a binary weak acid and can be ionized in steps in water. The first ionization equation is $H_2S\ rightleftharpoons H ^ ++ HS ^ - $, and the second ionization equation is $HS ^ -\ rightleftharpoons H ^ ++ S ^ {2 -} $.
Due to the excess of potassium hydroxide solution, a large number of hydroxide ions ($OH ^ - $) in the solution neutralize with hydrogen ions ionized from hydrogen sulfide ($H ^ + $). First, hydrogen ions ionized from hydrogen sulfide react with hydroxide ions in the first step, and the ionic equation is $H ^ ++ OH ^ - = H_2O $, which prompts the ionization equilibrium of hydrogen sulfide to shift to the right. Then, the generated $HS ^ - $continues to react with hydroxide ions, and the ionic equation is $HS ^ - + OH ^ - = S ^ {2 - } + H_2O $.
The chemical equation for the total reaction is $H_2S + 2KOH = K_2S + 2H_2O $, and the ionic equation is $H_2S + 2OH ^ - = S ^ {2 - } + 2H_2O $. The reaction results in the formation of potassium sulfide ($K_2S $) and water ($H_2O $). Potassium sulfide exists in solution in the form of potassium ions ($K ^ + $) and sulfur ions ($S ^ {2 -} $). This reaction reflects the essence of acid-base neutralization, which is a typical reaction of hydrogen sulfide as an acid gas with strong base potassium hydroxide.
Hydrogen sulfide is also a gas with rotten egg odor. When this gas is slowly introduced into excess potassium hydroxide solution, the two chemically react.
Potassium hydroxide is a strong base, and the concentration of hydroxide ions ($OH ^ - $) in its solution is quite high. Hydrogen sulfide ($H_2S $) is a binary weak acid and can be ionized in steps in water. The first ionization equation is $H_2S\ rightleftharpoons H ^ ++ HS ^ - $, and the second ionization equation is $HS ^ -\ rightleftharpoons H ^ ++ S ^ {2 -} $.
Due to the excess of potassium hydroxide solution, a large number of hydroxide ions ($OH ^ - $) in the solution neutralize with hydrogen ions ionized from hydrogen sulfide ($H ^ + $). First, hydrogen ions ionized from hydrogen sulfide react with hydroxide ions in the first step, and the ionic equation is $H ^ ++ OH ^ - = H_2O $, which prompts the ionization equilibrium of hydrogen sulfide to shift to the right. Then, the generated $HS ^ - $continues to react with hydroxide ions, and the ionic equation is $HS ^ - + OH ^ - = S ^ {2 - } + H_2O $.
The chemical equation for the total reaction is $H_2S + 2KOH = K_2S + 2H_2O $, and the ionic equation is $H_2S + 2OH ^ - = S ^ {2 - } + 2H_2O $. The reaction results in the formation of potassium sulfide ($K_2S $) and water ($H_2O $). Potassium sulfide exists in solution in the form of potassium ions ($K ^ + $) and sulfur ions ($S ^ {2 -} $). This reaction reflects the essence of acid-base neutralization, which is a typical reaction of hydrogen sulfide as an acid gas with strong base potassium hydroxide.
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