why is HS- a stronger BL base compared to HSO4
In a series of oxybases with the same central atom, the base with more O atoms is stronger.
In a series of oxybases with the same central atom, the base with less O atoms is stronger.
Since H2SO4 is one of the seven strong acids, HSO4- is a negligible base.
H2SO4 is a stronger acid than H2S, so HS- is the stronger conjugate base.
Since H2S is one of the seven strong acids, HS- is a negligible base.
H2S is a stronger acid than H2SO4, so HSO4- is the stronger conjugate base.
i chose the second third and fourth but it wasa wrong. please help!
Well, I hate to break it to you, but the best way to explain this is through a little chemistry humor. Here goes:
HS- is a stronger base compared to HSO4- because HS- has a better sense of basicity. You see, while HSO4- might have more O atoms, it seems to have a serious case of "Oxygen envy." It's always comparing itself to other bases with more O atoms and feeling inadequate. Meanwhile, HS- is just chillin' with its lone S atom, confident in its basicity. So, in the world of oxybases, having more O atoms doesn't automatically make you stronger. HS- embraces its simplicity and stands tall as a stronger base. Keep in mind, this is just a fun way to remember the concept. Good luck with your chemistry studies!
I apologize for the confusion. The correct statement is:
In a series of oxybases with the same central atom, the base with more O atoms is stronger.
So, the correct answer is: "In a series of oxybases with the same central atom, the base with more O atoms is stronger."
HS- is a stronger base compared to HSO4- because HS- has fewer oxygen atoms compared to HSO4-.
I can help you understand why HS- is a stronger base compared to HSO4-.
In the given options, the correct statement is "Since H2S is one of the seven strong acids, HS- is a negligible base."
To understand why, we need to consider the acid-base properties of the compounds involved.
H2S (hydrogen sulfide) and H2SO4 (sulfuric acid) are both acids, but they differ in their strengths as acids. H2S is a weak acid, while H2SO4 is a strong acid.
When an acid donates a proton (H+) to a base, it forms its conjugate base. Therefore, the conjugate base of H2S is HS-, and the conjugate base of H2SO4 is HSO4-.
In general, a stronger acid will have a weaker conjugate base. This means that the conjugate base of a stronger acid will be less likely to accept a proton and, therefore, will be a weaker base.
Since H2SO4 is a strong acid, its conjugate base, HSO4-, is a very weak base. On the other hand, H2S is a weak acid, and its conjugate base, HS-, is a stronger base than HSO4-.
Therefore, HS- is a stronger base compared to HSO4-.
It is important to note that the number of oxygen atoms in oxybases does not determine their relative strengths as bases. Rather, it is the strength of the acid from which the conjugate base is derived that plays a crucial role in determining the strength of the base.