Can anyone help me find an answer to the question above?
I'm planning exposure experiments with the use of hydrogen sulfide in the levels observed for natural environment to observe bivalve biochemical response to this toxic gas.
And what is the best way to carry out this experiment in small (e.g. 2 litre) containers to comply with health safety rules in a laboratory?
Thanks in advance!
Have a look at previous discussions using the same approach, see:
https://www.researchgate.net/post/Anyone_could_tell_me_the_actual_state_of_Na2S_in_water
https://www.researchgate.net/post/How_can_I_prepare_a_1_M_solution_of_sodium_sulphide_flakes_Na2SxH2O_assay_ex_s_315
https://www.chemicalforums.com/index.php?topic=3156.0
I think you have to check the reaction formula, the balancing it.
Sodium sulfide is expected to undergo partial hydrolysis: (i) Na2S + H2O ⇌ NaOH + NaHS; (ii) NaHS + H2O ⇌ NaOH + H2S; (iii or i + ii) Na2S + 2H2O ⇌ 2NaOH + H2S. H2S is a weak acid that dissociates into its ions HS- (bisulfide) and S2- (sulfide): (iv) H2S + H2O ⇌ HS- + H3O+; (v) HS- + H2O ⇌ S2- + H3O+; for pKa1 and pKa2 cf. (e.g.) (*). NaOH is a strong base that entirely dissociates. H2S concentration is very small except if the solution is significantly acidified. Evaporation of H2S from solution should otherwise be neglectable, because the solution would be rather basic.
Acidification should be prevented whenever possible and cautiously considered for the appropriate level of laboratory safety awareness.
(*)Article Chemical Foundations of Hydrogen Sulfide Biology
About the hydrate ― You may want to check my post at: https://www.researchgate.net/post/How_to_calculate_solubility_of_hydrated_inorganic_salts
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