If the concentration of a sample of aqueous hydrosulfric acid is 0.050 mol/L then the hydronium ion concentration is and the pOH of the solution is
The chemical equation for the dissociation of hydrosulfric acid (H2S) in water is:
H2S + H2O ⇌ H3O+ + HS-
From the equation, we can see that for every molecule of H2S that dissociates, one hydronium ion (H3O+) is produced. Therefore, the concentration of hydronium ions is equal to the concentration of hydrosulfric acid.
Thus, the hydronium ion concentration is 0.050 mol/L.
To find the pOH of the solution, we can use the equation:
pOH = -log[OH-]
Since hydrosulfric acid is a weak acid, we can assume that it does not significantly contribute to the hydroxide ion concentration. Therefore, we can assume that the concentration of hydroxide ions (OH-) is negligible.
In this case, the pOH of the solution would be equal to 14 (the pOH + pH of water) since the concentration of hydroxide ions is 0.
Therefore, the pOH of the solution is 14.