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Mithoron
Mithoron
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Tweeted twitter.com/#!/StackChemistry/status/453308960272306176
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buckminst
buckminst
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Why do only certainlycertain acids disassociate in water?

I understand that most acids are weak acids, i.e. they do not fully disassociate in solution. However, certain acids, such as H2SO4$\ce{H2SO4}$, do. I have been unable to foundfind out what the defining characteristic is that differentiates strong acids from weak ones.

For example, HCl is strong, yet both HF and HBr are weak (even though they're based on halogens as well). Shouldn't HF be even stronger?

What characteristic makes only a select few acids fully disassociate (and hence belong to the strong acid group)?

Why do only certainly acids disassociate in water?

I understand that most acids are weak acids, i.e. they do not fully disassociate in solution. However, certain acids, such as H2SO4 do. I have been unable to found out what the defining characteristic is that differentiates strong acids from weak ones.

For example, HCl is strong, yet both HF and HBr are weak (even though they're based on halogens as well). Shouldn't HF be even stronger?

What characteristic makes only a select few acids fully disassociate (and hence belong to the strong acid group)?

Why do only certain acids disassociate in water?

I understand that most acids are weak acids, i.e. they do not fully disassociate in solution. However, certain acids, such as $\ce{H2SO4}$, do. I have been unable to find out what the defining characteristic is that differentiates strong acids from weak ones.

For example, HCl is strong, yet both HF and HBr are weak (even though they're based on halogens as well). Shouldn't HF be even stronger?

What characteristic makes only a select few acids fully disassociate (and hence belong to the strong acid group)?

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Just_a_fool
Just_a_fool
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Why do only certainly acids disassociate in water?

I understand that most acids are weak acids, i.e. they do not fully disassociate in solution. However, certain acids, such as H2SO4 do. I have been unable to found out what the defining characteristic is that differentiates strong acids from weak ones.

For example, HCl is strong, yet both HF and HBr are weak (even though they're based on halogens as well). Shouldn't HF be even stronger?

What characteristic makes only a select few acids fully disassociate (and hence belong to the strong acid group)?