Which of the following is NOT soluble in water? A) NaCl B) KBr C) CH3CH2OH D) HCl E) C6H6 and how do i know?

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Which of the following is NOT soluble in water? A) NaCl B) KBr C) CH3CH2OH D) HCl E) C6H6 and how do i know?

Chemistry
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i know for sure it's not A
its C6H6 (benzene)
since when did you go green o.O

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Other answers:

and why do you say so/
yesterday
why do i say its benzene?
yes...how would you know?
im thinking it would have something to do with adhesion and cohesion? or no?
ok KBr is a soluble salt - an ionic compound ch3ch2oh is alcohol - it mixes well with my whisky benzene is a liquid which if you add to water forms a separate layer its an aromatic organic compound
ok...assuming i have no idea what you just said and i lack the experience to think like that...how else can i know?
hmm - well all i can say its a hydrocarbon which are not usually soluble in water.
im thinking it has something to do with cohesion-adhesion or hydrogen bonding or IMFA or something >.<
im so confused
yes - benzene would not take part in hydrogen bonding - that might be it - the molecule is hexagonal and very stable. sorry i can't be of more help
why do you say stable? and what does stability have anything to do with h-bonding?
benzene does not react with water at room temperature and only reacts with strong reagents at elevated temperatures the hexagonal arrangement makes for strong bonding.
well im gonna need a more general answer :(
what makes a compound not react with water
in alcohol for instance the hydrogen in OH bit is partially charge and attacks the H3O ion in the water. this can't happen with benzene
*attracts not attacks
gotta go now - my chemistry knowledge is pretty rusty I'm afraid
aww ok
I think It is C6H6 I think that is right :O
HOW to know which it is? im not really interested what the answer is
why not just use a solubility table? most textbooks are provided witt one in the appendix...
this is for a quiz...we dont have books in quizzes...i need to know HOW
...
am i allowed answering this?
what do you mean?
am i allowed answerign things related to marked papers?
this isnt a marked paper
im trying to review for my quiz in a few hours
what i was saying was that in our quiz we dont have books with solubilty table thingies so i shouldnt rely on it
anyway my question is just "HOW TO KNOW WHICH COMPUOUND IS SOLUBLE AND WHICH IS NOT"
Wow.
?
Goodluck :D
lol :p
I was provided a solubility charts eh, for my examination.... http://en.wikipedia.org/wiki/Solubility_chart
but without a solubility chart...how to know?
i think it was related to the ions and charges tho. to figure it out
im assuming it has something to do with hydrogen bonding or something
but none of the elements are ions o.O
Ahem. Wikipedia is my source. Please do not quote me on this.
Solubility of ionic compounds in water Main article: Solubility chart Main article: Solubility table Some ionic compounds (salts) dissolve in water, which arises because of the attraction between positive and negative charges (see: solvation). For example, the salt's positive ions (e.g. Ag+) attract the partially negative oxygens in H2O. Likewise, the salt's negative ions (e.g. Cl−) attract the partially positive hydrogens in H2O. Note: oxygen is partially negative because it is more electronegative than hydrogen, and vice-versa (see: chemical polarity). AgCl(s) Ag+(aq) + Cl−(aq) However, there is a limit to how much salt can be dissolved in a given volume of water. This amount is given by the solubility product, Ksp. This value depends on the type of salt (AgCl vs. NaCl, for example), temperature, and the common ion effect. One can calculate the amount of AgCl that will dissolve in 1 liter of water, some algebra is required. Ksp = [Ag+] × [Cl−] (definition of solubility product) Ksp = 1.8 × 10−10 (from a table of solubility products) [Ag+] = [Cl−], in the absence of other silver or chloride salts, [Ag+]2 = 1.8 × 10−10 [Ag+] = 1.34 × 10−5 The result: 1 liter of water can dissolve 1.34 × 10−5 moles of AgCl(s) at room temperature. Compared with other types of salts, AgCl is poorly soluble in water. In contrast, table salt (NaCl) has a higher Ksp and is, therefore, more soluble. Soluble Insoluble Group I and NH4+ compounds Carbonates (Except Group I, NH4+ and uranyl compounds) Nitrates Sulfites (Except Group I and NH4+ compounds) Acetates (Ethanoates) (Except Ag+ compounds) Phosphates (Except Group I and NH4+ compounds) Chlorides (Chlorates and Perchlorates), bromides and iodides (Except Ag+, Pb2+, Cu+ and Hg22+) Hydroxides and oxides (Except Group I, NH4+, Ba2+, Sr2+ and Tl+) Sulfates (Except Ag+, Pb2+, Ba2+, Sr2+ and Ca2+) Sulfides (Except Group I, Group II and NH4+ compounds) Hydroxides (Only with (aq) Ba2+, Li+, Na+, K+, Rb+, Cs+, Fr+ )
http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water
hmm so it's ion induced dipole huh
wonder how i'll know when it happens :/
possibly the molecule's attraction to the hydrogen in water makes it more soluble?
how would i know that by llooking at the compounds?
maybe not by looking at the compounds, but the periodic table?
what do you mean?
wait..that's electronegativity, charges and such...
yeah...
wait...
For example, the salt's positive ions (e.g. Ag+) attract the partially negative oxygens in H2O. Likewise, the salt's negative ions (e.g. Cl−) attract the partially positive hydrogens in H2O. Note: oxygen is partially negative because it is more electronegative than hydrogen, and vice-versa (see: chemical polarity). AgCl(s) Ag+(aq) + Cl−(aq)
However, there is a limit to how much salt can be dissolved in a given volume of water. This amount is given by the solubility product, Ksp. This value depends on the type of salt (AgCl vs. NaCl, for example), temperature, and the common ion effect. One can calculate the amount of AgCl that will dissolve in 1 liter of water, some algebra is required. Ksp = [Ag+] × [Cl−] (definition of solubility product) Ksp = 1.8 × 10−10 (from a table of solubility products)
The result: 1 liter of water can dissolve 1.34 × 10−5 moles of AgCl(s) at room temperature. Compared with other types of salts, AgCl is poorly soluble in water. In contrast, table salt (NaCl) has a higher Ksp and is, therefore, more soluble.
In relation to the points I posted: 1. Electronegativity DOEs play a role in solubility. 2. Using Ksp to find solubility. 3. Is a Ksp table provided?
with out looking it up i'm saying e is not soluble because it's molecular
what do you mean molecular?
it's a metal bonded to a non metal
you mean an ionic bond?
but NaCl is ionic too...
and wait...isnt c6h6 nonmetal + nonmetal?
c6h6 is a organic compound...
right and it wont disolbe in water
because it's nonmetal + nonmetal?
i think so...i don't think hexane, octane, etc dissolves easily in water...it just floats on top right
but HCl is non metal + nonmetal too...
hcl is a strong acid so it totaly ionizes
HCl is an acid.
and when added with water, loses its H, making it Cl2, and causes the water to become hydronium
but zbay said c6h6 does not dissolve because it's metal + nonmetal but NaCl is metal + nonmetal too if it's nonmetal + nonmetal HCl is nonmetal + nonmetal too
so what's the reason c6h6 does not dissolve?
i ment non metal non metal or molecular, and hcl is a strong acid making very soluble
Well, for one, It's got tons of hydrogen bonding...
because its molecular and because of that it doesn't disolve in water.
course, we may just be mixing this all up...I suggest the solubility table...
but why does HCl dissolve in water if it's molecular too?
It's simpler-less hydrogen bonds.
only 1, compared to 6 in c6h6
Hydrogen can act as a metal or non-metal so in this case it's acting as a metal
hydrogen bonding is a IMF and has nothing to do with that Tim
wats imf? it doesn't matter?
...it doesn't matter whether or not its metal does it? just the electronegativities?
an IMF is a intramolecular force and is responsible for how molecules behave around each other
isn't that important for solubility, as we are looking for the chemicals' ability to be dissolved in water. Whatever affects the forces must affect the solubility too right?
so how does IMF affect ths situation?
IMF has nothing to do with solubility, we are just trying to figure out if something will disolve here. So by a just remember that if the compound is molecular it doesn't disolve.
Polarity?
Nitrates, acetates, and ammonium though DO dissolve
in water
look i'm not trying to debate this all night the answer to the questoin is e in my opinion. There are other exeptions to these rules but the majority of the time just find the molecular compound and assume it wont be soluble. if you want to read about all the exeptions google solubilty rules
http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water
(Solubility table!)
-_- It has to do with the bonds/the charge of the polyatomic ions of the Chemicals. If you say otherwise you don't understand what happens when you dissolve a compound.
me? yeah i really dont
It has with the polarity of h2o pulling the positive ions from the compound
or the cations i should say
i didnt read all answers but you can take guidence in this rule: similar is soluble in similar by which i mean POLARITY!!! polar molecules will dissolve in water while non polar in non polar solutes like benzene, toluene, THF(tetra hydro furane)...
like dissolves like..
what does that mean?
i mean "like dissolves like" and btw..is nacl polar? isnt it ionic???
that means that salts like NaCl you mentioned will naturally be dissolved in water, other polar molecules like C2H5OH which have small organic groups and polar group will also dissolve in water cause in their case polarity of polar group (in this case OH) is significant, but for example fats and oils which are consisted of large organic chains will not dissolve in water (you can see that in soup where oil or fat floats on soup) but those will dissolve in nonpolar liquids (molecules) like toluene, benzene etc. because they are not polar...
for me, how to know the solubility are based on the BONDS. ionic compounds = soluble. covalent compounds = insoluble except in certain compounds, ex. HCl)

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