Hereof, is h2s an acid? The compound, H2S , is called hydrogen sulfide when it is in pure form but it is called hydrosulfuric acid when its acidic properties in aqueous solution are being discussed. One may also ask, why is h2s not dihydrogen sulfide? Because the molecular structure goes something like this: H-O-O-H In this case, the two oxygen form a single bond between each other , and this group is called a peroxide- or peroxo-group.
While H atom with S lacks H bonding and thus there bond can be broken very easily as compared to water. Hydrogen sulfide is a gaseous acid with a pKa of about 7. When you dissolve it into water it becomes hydrosulfuric acid , which is a weak acid. If you got it on your skin, it would be mildly irrirating. What is the pH of h2s? At pH 7, hydrogen sulfide is approximately 50 percent of the total dissolved sulfides; at pH 5, it is practically percent of the total; at pH 9, it is nearly all hydrosulfide ion.
Therefore the existence of hydrogen sulfide in sulfur-bearing waters is pH dependent. Is HCl a strong acid? A strong acid is an acid which is completely ionized in an aqueous solution. Hydrogen chloride HCl ionizes completely into hydrogen ions and chloride ions in water. A weak acid is an acid that ionizes only slightly in an aqueous solution. How many ppm h2s will kill you? Above Immediate loss of consciousness. Death is rapid, sometimes immediate.
Besides its poor warning properties, H2S is so dangerous because the level that can kill is much lower than that of many other toxic gases. What acid is hclo2? Chlorous acid is an inorganic compound with the formula HClO2. It is a weak acid. You are right that electronegativity is an important consideration but another factor that is also very important is size of the atom.
This allows the charge to be distributed over a larger volume of space, decreasing inter-electronic repulsions, providing greater stabilisation of the negative charge. However, the greater size decreases charge density, decreasing the strength of ion-dipole interactions between the anion and the surrounding water molecules.
Thus, the extent of solvation decreases for the larger anion. Electronegativity is defined as the ability of the atom to attract a bonding pair of electrons.
It merely serves as a proxy for the ability of the atom to stabilise negative charge. It should not be viewed as the most important factor that influences the atom's ability to stabilise negative charge. Also, mentioned in your answer, the strength of the bond formed with the larger atom with more diffuse orbitals decreases. Consolidating the above discussion, there are really two factors on each side of the table below. Perhaps, the distribution of charge increases very significantly and the bond energy also decreases significantly while the decrease in extent of solvation and the electronegativity exhibit a relatively less significant effect.
It would be great if someone is able to quantitatively show this It is not just electronegativity. You also have to look at how strongly the atom bonds to hydrogen. If a strong bond forms, it might convince the atom to act as a base even if it would be grumpy based on its electronegativity.
If only a weak bond forms, even an atom with relatively low electronegativity might balk at being protonated. It's due to favorable covalent overlap; take account of orbital sizes and nodes. Acidity is a bulk property - it depends on the medium where a substance acts as an acid. For example, ammonia, a weak base in aqueous medium, can be a strong base in another medium. But, when it comes to aqueous medium, many factors are taken into account to decide the strength of acidity.
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