Quantcast

Got Homework?

Connect with other students for help. It's a free community.

  • across
    MIT Grad Student
    Online now
  • laura*
    Helped 1,000 students
    Online now
  • Hero
    College Math Guru
    Online now

Here's the question you clicked on:

55 members online
  • 0 replying
  • 0 viewing

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?

  • one year ago
  • one year ago

  • This Question is Closed
  1. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    i know for sure it's not A

    • one year ago
  2. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    its C6H6 (benzene)

    • one year ago
  3. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    since when did you go green o.O

    • one year ago
  4. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    and why do you say so/

    • one year ago
  5. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    yesterday

    • one year ago
  6. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    why do i say its benzene?

    • one year ago
  7. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    yes...how would you know?

    • one year ago
  8. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    im thinking it would have something to do with adhesion and cohesion? or no?

    • one year ago
  9. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    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

    • one year ago
  10. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    ok...assuming i have no idea what you just said and i lack the experience to think like that...how else can i know?

    • one year ago
  11. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    hmm - well all i can say its a hydrocarbon which are not usually soluble in water.

    • one year ago
  12. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    im thinking it has something to do with cohesion-adhesion or hydrogen bonding or IMFA or something >.<

    • one year ago
  13. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    im so confused

    • one year ago
  14. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    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

    • one year ago
  15. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    why do you say stable? and what does stability have anything to do with h-bonding?

    • one year ago
  16. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    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.

    • one year ago
  17. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    well im gonna need a more general answer :(

    • one year ago
  18. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    what makes a compound not react with water

    • one year ago
  19. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    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

    • one year ago
  20. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    *attracts not attacks

    • one year ago
  21. cwrw238
    Best Response
    You've already chosen the best response.
    Medals 1

    gotta go now - my chemistry knowledge is pretty rusty I'm afraid

    • one year ago
  22. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    aww ok

    • one year ago
  23. SanjanaP
    Best Response
    You've already chosen the best response.
    Medals 1

    I think It is C6H6 I think that is right :O

    • one year ago
  24. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    HOW to know which it is? im not really interested what the answer is

    • one year ago
  25. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    why not just use a solubility table? most textbooks are provided witt one in the appendix...

    • one year ago
  26. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    this is for a quiz...we dont have books in quizzes...i need to know HOW

    • one year ago
  27. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    ...

    • one year ago
  28. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    am i allowed answering this?

    • one year ago
  29. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    what do you mean?

    • one year ago
  30. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    am i allowed answerign things related to marked papers?

    • one year ago
  31. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    this isnt a marked paper

    • one year ago
  32. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    im trying to review for my quiz in a few hours

    • one year ago
  33. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    what i was saying was that in our quiz we dont have books with solubilty table thingies so i shouldnt rely on it

    • one year ago
  34. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    anyway my question is just "HOW TO KNOW WHICH COMPUOUND IS SOLUBLE AND WHICH IS NOT"

    • one year ago
  35. GOODMAN
    Best Response
    You've already chosen the best response.
    Medals 0

    Wow.

    • one year ago
  36. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    ?

    • one year ago
  37. GOODMAN
    Best Response
    You've already chosen the best response.
    Medals 0

    Goodluck :D

    • one year ago
  38. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    lol :p

    • one year ago
  39. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    I was provided a solubility charts eh, for my examination.... http://en.wikipedia.org/wiki/Solubility_chart

    • one year ago
  40. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    but without a solubility chart...how to know?

    • one year ago
  41. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    i think it was related to the ions and charges tho. to figure it out

    • one year ago
  42. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    im assuming it has something to do with hydrogen bonding or something

    • one year ago
  43. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    but none of the elements are ions o.O

    • one year ago
  44. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    Ahem. Wikipedia is my source. Please do not quote me on this.

    • one year ago
  45. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    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+ )

    • one year ago
  46. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water

    • one year ago
  47. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    hmm so it's ion induced dipole huh

    • one year ago
  48. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    wonder how i'll know when it happens :/

    • one year ago
  49. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    possibly the molecule's attraction to the hydrogen in water makes it more soluble?

    • one year ago
  50. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    how would i know that by llooking at the compounds?

    • one year ago
  51. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    maybe not by looking at the compounds, but the periodic table?

    • one year ago
  52. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    what do you mean?

    • one year ago
  53. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    wait..that's electronegativity, charges and such...

    • one year ago
  54. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    yeah...

    • one year ago
  55. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    wait...

    • one year ago
  56. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    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)

    • one year ago
  57. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    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)

    • one year ago
  58. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    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.

    • one year ago
  59. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    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?

    • one year ago
  60. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    with out looking it up i'm saying e is not soluble because it's molecular

    • one year ago
  61. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    what do you mean molecular?

    • one year ago
  62. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    it's a metal bonded to a non metal

    • one year ago
  63. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    you mean an ionic bond?

    • one year ago
  64. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    but NaCl is ionic too...

    • one year ago
  65. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    and wait...isnt c6h6 nonmetal + nonmetal?

    • one year ago
  66. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    c6h6 is a organic compound...

    • one year ago
  67. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    right and it wont disolbe in water

    • one year ago
  68. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    because it's nonmetal + nonmetal?

    • one year ago
  69. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    i think so...i don't think hexane, octane, etc dissolves easily in water...it just floats on top right

    • one year ago
  70. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    but HCl is non metal + nonmetal too...

    • one year ago
  71. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    hcl is a strong acid so it totaly ionizes

    • one year ago
  72. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    HCl is an acid.

    • one year ago
  73. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    and when added with water, loses its H, making it Cl2, and causes the water to become hydronium

    • one year ago
  74. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    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

    • one year ago
  75. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    so what's the reason c6h6 does not dissolve?

    • one year ago
  76. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    i ment non metal non metal or molecular, and hcl is a strong acid making very soluble

    • one year ago
  77. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    Well, for one, It's got tons of hydrogen bonding...

    • one year ago
  78. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    because its molecular and because of that it doesn't disolve in water.

    • one year ago
  79. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    course, we may just be mixing this all up...I suggest the solubility table...

    • one year ago
  80. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    but why does HCl dissolve in water if it's molecular too?

    • one year ago
  81. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    It's simpler-less hydrogen bonds.

    • one year ago
  82. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    only 1, compared to 6 in c6h6

    • one year ago
  83. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    Hydrogen can act as a metal or non-metal so in this case it's acting as a metal

    • one year ago
  84. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    hydrogen bonding is a IMF and has nothing to do with that Tim

    • one year ago
  85. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    wats imf? it doesn't matter?

    • one year ago
  86. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    ...it doesn't matter whether or not its metal does it? just the electronegativities?

    • one year ago
  87. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    an IMF is a intramolecular force and is responsible for how molecules behave around each other

    • one year ago
  88. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    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?

    • one year ago
  89. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    so how does IMF affect ths situation?

    • one year ago
  90. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    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.

    • one year ago
  91. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    Polarity?

    • one year ago
  92. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    Nitrates, acetates, and ammonium though DO dissolve

    • one year ago
  93. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    in water

    • one year ago
  94. zbay
    Best Response
    You've already chosen the best response.
    Medals 0

    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

    • one year ago
  95. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water

    • one year ago
  96. NotTim
    Best Response
    You've already chosen the best response.
    Medals 1

    (Solubility table!)

    • one year ago
  97. Outkast3r09
    Best Response
    You've already chosen the best response.
    Medals 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.

    • one year ago
  98. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    me? yeah i really dont

    • one year ago
  99. Outkast3r09
    Best Response
    You've already chosen the best response.
    Medals 0

    It has with the polarity of h2o pulling the positive ions from the compound

    • one year ago
  100. Outkast3r09
    Best Response
    You've already chosen the best response.
    Medals 0

    or the cations i should say

    • one year ago
  101. Kryten
    Best Response
    You've already chosen the best response.
    Medals 1

    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)...

    • one year ago
  102. foodscientist
    Best Response
    You've already chosen the best response.
    Medals 0

    like dissolves like..

    • one year ago
  103. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    what does that mean?

    • one year ago
  104. lgbasallote
    Best Response
    You've already chosen the best response.
    Medals 1

    i mean "like dissolves like" and btw..is nacl polar? isnt it ionic???

    • one year ago
  105. Kryten
    Best Response
    You've already chosen the best response.
    Medals 1

    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...

    • one year ago
  106. am01656
    Best Response
    You've already chosen the best response.
    Medals 0

    for me, how to know the solubility are based on the BONDS. ionic compounds = soluble. covalent compounds = insoluble except in certain compounds, ex. HCl)

    • one year ago
    • Attachments:

See more questions >>>

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
  • 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.

This is the testimonial you wrote.
You haven't written a testimonial for Owlfred.