Strong, weak, or nonelectrolyte? how will I know? propyl amine, potassium iodide and carbonic acid, what kind of electrolyte are they?

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Strong, weak, or nonelectrolyte? how will I know? propyl amine, potassium iodide and carbonic acid, what kind of electrolyte are they?

Chemistry
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write these all out as chemical compounds first

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ok.. propyl amine: \(CH_3CH_2CH_2NH_2\) potassium iodide: KI and carbonic acid: \(H_2CO_3\)
then..?
I think KI is a strong electrolyte.. because of K+ and I-
@owlet electrolytes usually produce ions in solution
Im not too sure about propyl amine, but if you look at it's structure you know that \(\sf CH_3CH_2CH_2\mathbf{NH_2}\) have hydrogen bonds, and hydrogen bonds take a lot of energy to break. You are right about \(\sf KI\), therefore it's a strong electrolyte because it has an ionic bond, and ionic bonds are soluble in water. for Carbonic Acid, \(\sf H_2CO_3\), ask yourself whether it's a strong acid, if it's a strong acid, then it's a strong electrolyte
I think acids are also considered electrolytes. and their strength depends on how many H+ ions are produced.
for acids and bases, the strength of their electrolytes depends on whether theyre a strong acid, or a strong base
okay.. just wanted to confirm.. if a substance is a strong acid/base then they are strong electrolytes?
yeah, because that means more ions are produced
Acetate, \(\sf HC_2H_3O_2\) is a weak electrolyte compared to let's say... nitric acid, \(\sf HNO_3\)
what about organic compounds, like glucose? they have H bonds also..?
|dw:1443922500887:dw| @owlet question to you is that compound above hexane would that be considered an electrolyte?
and why?
i think it is nonelectrolyte because.. it doesn't ionize in water..?
yep @owlet another one, which one is a better electrolyte and why? |dw:1443922689755:dw|
I'm not sure about that one
both of them will ionize, aren't they?
=]
acetic acid is a strong acid, so it should be the one i think
what does acidic strength mean? and how does this relate to electrolyte strength?
hmm acidic strength has something to do with loosing H+ ? it is related to electrolyte strength because i think.. if the acid is strong, it will ionize completely(loose all H+) .. i don't know anymore
but acetic acid and sulfuric acid are both strong acids though??
yep strong acid will produce more H+
@owlet acetic acid is a weak acid, sulfuric acid is a strong acid
so based off of this which would be the better electrolyte?
ohh so it is sulfuric acid? quick question.... i know this may sound dumb.. but why is acetic acid a weak one?
yep =]
well because it loses some of it's protons, not all. have you heard of something called Ka, acid dissociation constant. NOT pKA \[HA --> H ^{+} + A ^{-} | Ka = \frac{ [H ^{+}][A ^{-}] }{ [KA] } \]
yeah I remember doing that. I completely forgot everything, that's why I'm revising everything :3
so @owlet would a strong acid have a High Ka or low, and how could you tell this from looking at the equation?
They should have a high Ka. The larger the Ka, the larger the [H+] ?
If [H+] is high, then it means the acid can donate more?
=] yep
like unfortunately, I was told in my chem classes to just memorize that H2SO4 is a strong acid, I don't like that but that's what I was told lol. but it's a strong acid b/c it's Ka is high. which means it's pKA meaning -log[Ka] will be small.
yes! ok i think i'm getting it now.. yeah same thing, we have to like memorize a table of strong & weak acids and bases before doing the solving part. Probably that's the reason why forgot everything lol let me try another substance.. carbonic acid... will it be weak?
In my classes they taught me that well yeah, These are your strong acids H2SO4 HNO3 HCL HBr HI H3PO4 i think i'm missing one. everything else is weak
how about HF?
that's a weak acid
oh yeah one more thing, before i closed this question.. how about alcohols also?
F- i think is very unstable and it's going to react readily
I'm not too sure about alcohols but I think they would be weak electrolytes
at least in water though could be different
F is super negative so it will attach to H+ more than the other group 17 i think, so probably it is weak.. hmm okay, i will try to read more to find out about alcohols. Thanks a lot for the help! :)
no problem
\(\color{#0cbb34}{\text{Originally Posted by}}\) @Photon336 In my classes they taught me that well yeah, These are your strong acids H2SO4 HNO3 HCL HBr HI H3PO4 i think i'm missing one. everything else is weak \(\color{#0cbb34}{\text{End of Quote}}\) You were pissing perchloric acid i believe, \(\sf HClO_4\)
\(\sf H_3PO_4\) is a weak acid :P
this is what happens when you just memorize stuff, I always forget one of them BTW how do you quote lol? @Jhannybean
Ohh Jaynator has a script you add to chrome for OS that allows you quote, and post images in the drawing tool as well as use different colors when drawing things as well. I'll have to find the link to the script, or you can ask Nnesha :P
if you find it please send that to me!
sure thing!
since you guys are still here.... HNO2 vs.HNO3, which is a stronger one? HNO3 right?
nvm, got it

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