lgbasallote
  • lgbasallote
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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SOLVED
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schrodinger
  • schrodinger
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lgbasallote
  • lgbasallote
i know for sure it's not A
cwrw238
  • cwrw238
its C6H6 (benzene)
lgbasallote
  • lgbasallote
since when did you go green o.O

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lgbasallote
  • lgbasallote
and why do you say so/
cwrw238
  • cwrw238
yesterday
cwrw238
  • cwrw238
why do i say its benzene?
lgbasallote
  • lgbasallote
yes...how would you know?
lgbasallote
  • lgbasallote
im thinking it would have something to do with adhesion and cohesion? or no?
cwrw238
  • cwrw238
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
lgbasallote
  • lgbasallote
ok...assuming i have no idea what you just said and i lack the experience to think like that...how else can i know?
cwrw238
  • cwrw238
hmm - well all i can say its a hydrocarbon which are not usually soluble in water.
lgbasallote
  • lgbasallote
im thinking it has something to do with cohesion-adhesion or hydrogen bonding or IMFA or something >.<
lgbasallote
  • lgbasallote
im so confused
cwrw238
  • cwrw238
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
lgbasallote
  • lgbasallote
why do you say stable? and what does stability have anything to do with h-bonding?
cwrw238
  • cwrw238
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.
lgbasallote
  • lgbasallote
well im gonna need a more general answer :(
lgbasallote
  • lgbasallote
what makes a compound not react with water
cwrw238
  • cwrw238
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
cwrw238
  • cwrw238
*attracts not attacks
cwrw238
  • cwrw238
gotta go now - my chemistry knowledge is pretty rusty I'm afraid
lgbasallote
  • lgbasallote
aww ok
SanjanaP
  • SanjanaP
I think It is C6H6 I think that is right :O
lgbasallote
  • lgbasallote
HOW to know which it is? im not really interested what the answer is
NotTim
  • NotTim
why not just use a solubility table? most textbooks are provided witt one in the appendix...
lgbasallote
  • lgbasallote
this is for a quiz...we dont have books in quizzes...i need to know HOW
NotTim
  • NotTim
...
NotTim
  • NotTim
am i allowed answering this?
lgbasallote
  • lgbasallote
what do you mean?
NotTim
  • NotTim
am i allowed answerign things related to marked papers?
lgbasallote
  • lgbasallote
this isnt a marked paper
lgbasallote
  • lgbasallote
im trying to review for my quiz in a few hours
lgbasallote
  • lgbasallote
what i was saying was that in our quiz we dont have books with solubilty table thingies so i shouldnt rely on it
lgbasallote
  • lgbasallote
anyway my question is just "HOW TO KNOW WHICH COMPUOUND IS SOLUBLE AND WHICH IS NOT"
anonymous
  • anonymous
Wow.
lgbasallote
  • lgbasallote
?
anonymous
  • anonymous
Goodluck :D
lgbasallote
  • lgbasallote
lol :p
NotTim
  • NotTim
I was provided a solubility charts eh, for my examination.... http://en.wikipedia.org/wiki/Solubility_chart
lgbasallote
  • lgbasallote
but without a solubility chart...how to know?
NotTim
  • NotTim
i think it was related to the ions and charges tho. to figure it out
lgbasallote
  • lgbasallote
im assuming it has something to do with hydrogen bonding or something
lgbasallote
  • lgbasallote
but none of the elements are ions o.O
NotTim
  • NotTim
Ahem. Wikipedia is my source. Please do not quote me on this.
NotTim
  • NotTim
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+ )
NotTim
  • NotTim
http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water
lgbasallote
  • lgbasallote
hmm so it's ion induced dipole huh
lgbasallote
  • lgbasallote
wonder how i'll know when it happens :/
NotTim
  • NotTim
possibly the molecule's attraction to the hydrogen in water makes it more soluble?
lgbasallote
  • lgbasallote
how would i know that by llooking at the compounds?
NotTim
  • NotTim
maybe not by looking at the compounds, but the periodic table?
lgbasallote
  • lgbasallote
what do you mean?
NotTim
  • NotTim
wait..that's electronegativity, charges and such...
lgbasallote
  • lgbasallote
yeah...
NotTim
  • NotTim
wait...
NotTim
  • NotTim
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)
NotTim
  • NotTim
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)
NotTim
  • NotTim
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.
NotTim
  • NotTim
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?
anonymous
  • anonymous
with out looking it up i'm saying e is not soluble because it's molecular
lgbasallote
  • lgbasallote
what do you mean molecular?
anonymous
  • anonymous
it's a metal bonded to a non metal
lgbasallote
  • lgbasallote
you mean an ionic bond?
lgbasallote
  • lgbasallote
but NaCl is ionic too...
lgbasallote
  • lgbasallote
and wait...isnt c6h6 nonmetal + nonmetal?
NotTim
  • NotTim
c6h6 is a organic compound...
anonymous
  • anonymous
right and it wont disolbe in water
lgbasallote
  • lgbasallote
because it's nonmetal + nonmetal?
NotTim
  • NotTim
i think so...i don't think hexane, octane, etc dissolves easily in water...it just floats on top right
lgbasallote
  • lgbasallote
but HCl is non metal + nonmetal too...
anonymous
  • anonymous
hcl is a strong acid so it totaly ionizes
NotTim
  • NotTim
HCl is an acid.
NotTim
  • NotTim
and when added with water, loses its H, making it Cl2, and causes the water to become hydronium
lgbasallote
  • lgbasallote
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
lgbasallote
  • lgbasallote
so what's the reason c6h6 does not dissolve?
anonymous
  • anonymous
i ment non metal non metal or molecular, and hcl is a strong acid making very soluble
NotTim
  • NotTim
Well, for one, It's got tons of hydrogen bonding...
anonymous
  • anonymous
because its molecular and because of that it doesn't disolve in water.
NotTim
  • NotTim
course, we may just be mixing this all up...I suggest the solubility table...
lgbasallote
  • lgbasallote
but why does HCl dissolve in water if it's molecular too?
NotTim
  • NotTim
It's simpler-less hydrogen bonds.
NotTim
  • NotTim
only 1, compared to 6 in c6h6
anonymous
  • anonymous
Hydrogen can act as a metal or non-metal so in this case it's acting as a metal
anonymous
  • anonymous
hydrogen bonding is a IMF and has nothing to do with that Tim
NotTim
  • NotTim
wats imf? it doesn't matter?
NotTim
  • NotTim
...it doesn't matter whether or not its metal does it? just the electronegativities?
anonymous
  • anonymous
an IMF is a intramolecular force and is responsible for how molecules behave around each other
NotTim
  • NotTim
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?
lgbasallote
  • lgbasallote
so how does IMF affect ths situation?
anonymous
  • anonymous
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.
NotTim
  • NotTim
Polarity?
NotTim
  • NotTim
Nitrates, acetates, and ammonium though DO dissolve
NotTim
  • NotTim
in water
anonymous
  • anonymous
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
NotTim
  • NotTim
http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water
NotTim
  • NotTim
(Solubility table!)
anonymous
  • anonymous
-_- 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.
lgbasallote
  • lgbasallote
me? yeah i really dont
anonymous
  • anonymous
It has with the polarity of h2o pulling the positive ions from the compound
anonymous
  • anonymous
or the cations i should say
anonymous
  • anonymous
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)...
anonymous
  • anonymous
like dissolves like..
lgbasallote
  • lgbasallote
what does that mean?
lgbasallote
  • lgbasallote
i mean "like dissolves like" and btw..is nacl polar? isnt it ionic???
anonymous
  • anonymous
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...
anonymous
  • anonymous
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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