A community for students.
Here's the question you clicked on:
 0 viewing
lgbasallote
 4 years ago
Which of the following is NOT soluble in water?
A) NaCl B) KBr C) CH3CH2OH D) HCl E) C6H6
and how do i know?
lgbasallote
 4 years ago
Which of the following is NOT soluble in water? A) NaCl B) KBr C) CH3CH2OH D) HCl E) C6H6 and how do i know?

This Question is Closed

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1i know for sure it's not A

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1since when did you go green o.O

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1and why do you say so/

cwrw238
 4 years ago
Best ResponseYou've already chosen the best response.1why do i say its benzene?

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1yes...how would you know?

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1im thinking it would have something to do with adhesion and cohesion? or no?

cwrw238
 4 years ago
Best ResponseYou've already chosen the best response.1ok 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
 4 years ago
Best ResponseYou've already chosen the best response.1ok...assuming i have no idea what you just said and i lack the experience to think like that...how else can i know?

cwrw238
 4 years ago
Best ResponseYou've already chosen the best response.1hmm  well all i can say its a hydrocarbon which are not usually soluble in water.

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1im thinking it has something to do with cohesionadhesion or hydrogen bonding or IMFA or something >.<

cwrw238
 4 years ago
Best ResponseYou've already chosen the best response.1yes  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
 4 years ago
Best ResponseYou've already chosen the best response.1why do you say stable? and what does stability have anything to do with hbonding?

cwrw238
 4 years ago
Best ResponseYou've already chosen the best response.1benzene 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
 4 years ago
Best ResponseYou've already chosen the best response.1well im gonna need a more general answer :(

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1what makes a compound not react with water

cwrw238
 4 years ago
Best ResponseYou've already chosen the best response.1in 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
 4 years ago
Best ResponseYou've already chosen the best response.1gotta go now  my chemistry knowledge is pretty rusty I'm afraid

SanjanaP
 4 years ago
Best ResponseYou've already chosen the best response.1I think It is C6H6 I think that is right :O

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1HOW to know which it is? im not really interested what the answer is

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1why not just use a solubility table? most textbooks are provided witt one in the appendix...

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1this is for a quiz...we dont have books in quizzes...i need to know HOW

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1am i allowed answering this?

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1am i allowed answerign things related to marked papers?

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1this isnt a marked paper

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1im trying to review for my quiz in a few hours

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1what i was saying was that in our quiz we dont have books with solubilty table thingies so i shouldnt rely on it

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1anyway my question is just "HOW TO KNOW WHICH COMPUOUND IS SOLUBLE AND WHICH IS NOT"

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1I was provided a solubility charts eh, for my examination.... http://en.wikipedia.org/wiki/Solubility_chart

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1but without a solubility chart...how to know?

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1i think it was related to the ions and charges tho. to figure it out

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1im assuming it has something to do with hydrogen bonding or something

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1but none of the elements are ions o.O

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1Ahem. Wikipedia is my source. Please do not quote me on this.

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1Solubility 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 viceversa (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
 4 years ago
Best ResponseYou've already chosen the best response.1http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1hmm so it's ion induced dipole huh

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1wonder how i'll know when it happens :/

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1possibly the molecule's attraction to the hydrogen in water makes it more soluble?

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1how would i know that by llooking at the compounds?

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1maybe not by looking at the compounds, but the periodic table?

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1wait..that's electronegativity, charges and such...

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1For 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 viceversa (see: chemical polarity). AgCl(s) Ag+(aq) + Cl−(aq)

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1However, 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
 4 years ago
Best ResponseYou've already chosen the best response.1The 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
 4 years ago
Best ResponseYou've already chosen the best response.1In 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
 4 years ago
Best ResponseYou've already chosen the best response.0with out looking it up i'm saying e is not soluble because it's molecular

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1what do you mean molecular?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0it's a metal bonded to a non metal

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1you mean an ionic bond?

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1but NaCl is ionic too...

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1and wait...isnt c6h6 nonmetal + nonmetal?

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1c6h6 is a organic compound...

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0right and it wont disolbe in water

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1because it's nonmetal + nonmetal?

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1i think so...i don't think hexane, octane, etc dissolves easily in water...it just floats on top right

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1but HCl is non metal + nonmetal too...

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0hcl is a strong acid so it totaly ionizes

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1and when added with water, loses its H, making it Cl2, and causes the water to become hydronium

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1but 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
 4 years ago
Best ResponseYou've already chosen the best response.1so what's the reason c6h6 does not dissolve?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0i ment non metal non metal or molecular, and hcl is a strong acid making very soluble

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1Well, for one, It's got tons of hydrogen bonding...

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0because its molecular and because of that it doesn't disolve in water.

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1course, we may just be mixing this all up...I suggest the solubility table...

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1but why does HCl dissolve in water if it's molecular too?

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1It's simplerless hydrogen bonds.

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1only 1, compared to 6 in c6h6

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Hydrogen can act as a metal or nonmetal so in this case it's acting as a metal

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0hydrogen bonding is a IMF and has nothing to do with that Tim

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1wats imf? it doesn't matter?

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1...it doesn't matter whether or not its metal does it? just the electronegativities?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0an IMF is a intramolecular force and is responsible for how molecules behave around each other

NotTim
 4 years ago
Best ResponseYou've already chosen the best response.1isn'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
 4 years ago
Best ResponseYou've already chosen the best response.1so how does IMF affect ths situation?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0IMF 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
 4 years ago
Best ResponseYou've already chosen the best response.1Nitrates, acetates, and ammonium though DO dissolve

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0look 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
 4 years ago
Best ResponseYou've already chosen the best response.1http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0_ 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
 4 years ago
Best ResponseYou've already chosen the best response.1me? yeah i really dont

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0It has with the polarity of h2o pulling the positive ions from the compound

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0or the cations i should say

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0i 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
 4 years ago
Best ResponseYou've already chosen the best response.0like dissolves like..

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1what does that mean?

lgbasallote
 4 years ago
Best ResponseYou've already chosen the best response.1i mean "like dissolves like" and btw..is nacl polar? isnt it ionic???

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0that 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
 4 years ago
Best ResponseYou've already chosen the best response.0for me, how to know the solubility are based on the BONDS. ionic compounds = soluble. covalent compounds = insoluble except in certain compounds, ex. HCl)
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.