Why do nonpolar solvents dissolve in nonpolar solutes?
Q. I didn't get solvents and solutes confused did I? Either way, thank you very much! <3
Asked by somrp2 - Sat Feb 28 02:37:29 2009 - - 1 Answers - 0 Comments
A. You did get them confused (solvents dissolve the solutes), however that doesn't much affect the questions so to continue: The act of dissolving really depends on 4 interactions: (1): The strength of the intermolecular forces between two solvent molecules (2): The strength of the intermolecular forces between two solute molecules. (3): The strength of the intermolecular forces between a solvent molecule and a solute molecule. (4): Entropy, which more or less states that all other things being equal, things like to mix. Overall, to have something dissolve the average effects of (1) and (2) need to be less than the effects of (3) and (4). So, when you have a polar solvent and a non-polar solute, the polar molecules have a much stronger… [cont.]
Answered by Mef - Sat Feb 28 02:50:54 2009
Q. I didn't get solvents and solutes confused did I? Either way, thank you very much! <3
Asked by somrp2 - Sat Feb 28 02:37:29 2009 - - 1 Answers - 0 Comments
A. You did get them confused (solvents dissolve the solutes), however that doesn't much affect the questions so to continue: The act of dissolving really depends on 4 interactions: (1): The strength of the intermolecular forces between two solvent molecules (2): The strength of the intermolecular forces between two solute molecules. (3): The strength of the intermolecular forces between a solvent molecule and a solute molecule. (4): Entropy, which more or less states that all other things being equal, things like to mix. Overall, to have something dissolve the average effects of (1) and (2) need to be less than the effects of (3) and (4). So, when you have a polar solvent and a non-polar solute, the polar molecules have a much stronger… [cont.]
Answered by Mef - Sat Feb 28 02:50:54 2009
How do you get a qualitative idea of how certain solutes dissolve in certain solvents?
Q. please help!!!
Asked by chetz - Wed Nov 29 20:50:03 2006 - - 1 Answers - 0 Comments
A. Like dissolves like...where you're looking at polarity. Covalently bonded solutes usually dissovle in covalently bonded solvents, but not in very polar things like water. Salts, which are ionically bonded, require very polar solvents (like water or liquid ammonia). Polar functional groups on solute molecules mean you need similar polar groups on your solvent molecules. Non-polar solutes like non-polar solvents.
Answered by rb42redsuns - Wed Nov 29 21:28:22 2006
Q. please help!!!
Asked by chetz - Wed Nov 29 20:50:03 2006 - - 1 Answers - 0 Comments
A. Like dissolves like...where you're looking at polarity. Covalently bonded solutes usually dissovle in covalently bonded solvents, but not in very polar things like water. Salts, which are ionically bonded, require very polar solvents (like water or liquid ammonia). Polar functional groups on solute molecules mean you need similar polar groups on your solvent molecules. Non-polar solutes like non-polar solvents.
Answered by rb42redsuns - Wed Nov 29 21:28:22 2006
About solutes and solvents.?
Q. It is usually observed that solutes dissolve in a definite amount in a solvent at a particular temperature.Is there any solute which dissolves to a infinite amount in a solvent the solute might be a liquid but it should not be miscible[the volume of solvent shouldnt increase.] tell me some such solutes and solvents.
Asked by hash - Wed Jul 26 05:38:30 2006 - - 5 Answers - 0 Comments
A. The volume of any solvent is affected by addition of solutes in moderate quantities, even more so in "infinite amounts". Try adding sugar to water and observe the change in volume. There may even be a decrease in volume for small quantities, depending on the temperature and special structure of the solvent, but generally adding substance with a volume of its own will affect the total volume by adding to it. Demanding that a solute liquid should not be miscible is sort of paradoxical if you want "infinite amounts" to be dissolved.
Answered by jorganos - Wed Jul 26 06:02:22 2006
Q. It is usually observed that solutes dissolve in a definite amount in a solvent at a particular temperature.Is there any solute which dissolves to a infinite amount in a solvent the solute might be a liquid but it should not be miscible[the volume of solvent shouldnt increase.] tell me some such solutes and solvents.
Asked by hash - Wed Jul 26 05:38:30 2006 - - 5 Answers - 0 Comments
A. The volume of any solvent is affected by addition of solutes in moderate quantities, even more so in "infinite amounts". Try adding sugar to water and observe the change in volume. There may even be a decrease in volume for small quantities, depending on the temperature and special structure of the solvent, but generally adding substance with a volume of its own will affect the total volume by adding to it. Demanding that a solute liquid should not be miscible is sort of paradoxical if you want "infinite amounts" to be dissolved.
Answered by jorganos - Wed Jul 26 06:02:22 2006
why is the solute first dissolved in a small quantity of solvent before filling the volumetric flask?
Q. why is the solute first dissolved in a small quantity of solvent before filling the volumetric flask?
Asked by $$$Arashi$$$ - Tue Sep 8 00:06:57 2009 - - 1 Answers - 0 Comments
Q. why is the solute first dissolved in a small quantity of solvent before filling the volumetric flask?
Asked by $$$Arashi$$$ - Tue Sep 8 00:06:57 2009 - - 1 Answers - 0 Comments
Why do the rate of solubility and rate of dissolving have different factors?
Q. If solubility is the measure of how much solute can dissolve in a solvent, and dissolving is the action of a solute mixing into a solvent, then they're almost alike, right? So solubility is the measure, and dissolving is the action. Why do they have different factors that influence? I'm so confused! ... Could someone please explain it all clearly to me? I'd really appreciate it!
Asked by Hikari - Tue Aug 7 22:28:23 2007 - - 1 Answers - 0 Comments
A. I don't have a "clean" answer to this. You need to realize that there time is the problem here. While the solubility measures the total amount that can dissolve, it does not tell you how long it takes to accomplish this. The, dissolving has a time component, too - and is highly dependent on surface area that is exposed to the solvent. So, there is no a prioiri reason why the two should behave in similar manners even though they may measure similar things.
Answered by KennyB - Tue Aug 7 22:40:25 2007
Q. If solubility is the measure of how much solute can dissolve in a solvent, and dissolving is the action of a solute mixing into a solvent, then they're almost alike, right? So solubility is the measure, and dissolving is the action. Why do they have different factors that influence? I'm so confused! ... Could someone please explain it all clearly to me? I'd really appreciate it!
Asked by Hikari - Tue Aug 7 22:28:23 2007 - - 1 Answers - 0 Comments
A. I don't have a "clean" answer to this. You need to realize that there time is the problem here. While the solubility measures the total amount that can dissolve, it does not tell you how long it takes to accomplish this. The, dissolving has a time component, too - and is highly dependent on surface area that is exposed to the solvent. So, there is no a prioiri reason why the two should behave in similar manners even though they may measure similar things.
Answered by KennyB - Tue Aug 7 22:40:25 2007
Solvents and Solutes?what?! help!?
Q. For each of the solvents below, choose the solute that will dissolve to a greater extent at room temp. Solvent Solute Choices Water (H2O) CHCl3 or CCl4 Ethanol (C2H5OH) KOH or BBr3 Methaol (CH3OH) BrF3 or SbF5 Pentane (C5H12) SF4 or SF6 Propanol (C3H7OH) C6H14 or H2O If you have the answer please please tell me how you got it!? thanks!
Asked by Tracey Lee - Thu Mar 1 20:49:00 2007 - - 1 Answers - 1 Comments
A. the basic solubility rule is "like dissolves like" 1) CH3Cl has some polarity and will dissolve more in polar water than nonpolar CCl4 2) KOH is ionic and will dissolve more in polar ethanol than nonpolar BBr3 3) BrF3 has some polarity and will dissolve more in polar methanol than nonpolar SbF5 4) SF6 is nonpolar and will dissolve more in nonpolar pentane than slightly polar SF4 5) H2O is polar and will dissolve more in polar propanol than nonpolar C6H14
Answered by chem geek - Thu Mar 1 21:11:51 2007
Q. For each of the solvents below, choose the solute that will dissolve to a greater extent at room temp. Solvent Solute Choices Water (H2O) CHCl3 or CCl4 Ethanol (C2H5OH) KOH or BBr3 Methaol (CH3OH) BrF3 or SbF5 Pentane (C5H12) SF4 or SF6 Propanol (C3H7OH) C6H14 or H2O If you have the answer please please tell me how you got it!? thanks!
Asked by Tracey Lee - Thu Mar 1 20:49:00 2007 - - 1 Answers - 1 Comments
A. the basic solubility rule is "like dissolves like" 1) CH3Cl has some polarity and will dissolve more in polar water than nonpolar CCl4 2) KOH is ionic and will dissolve more in polar ethanol than nonpolar BBr3 3) BrF3 has some polarity and will dissolve more in polar methanol than nonpolar SbF5 4) SF6 is nonpolar and will dissolve more in nonpolar pentane than slightly polar SF4 5) H2O is polar and will dissolve more in polar propanol than nonpolar C6H14
Answered by chem geek - Thu Mar 1 21:11:51 2007
identify the solvents, solutions and solutes in this solution?
Q. a mixture of syrup is made by dissolving sugar in water in a beaker. identify the solvent, solution and solute solvent = solution = solute = thanks for you time and help x
Asked by . . .pInKii PoOpEr. . . - Sat Apr 12 06:44:08 2008 - - 4 Answers - 0 Comments
A. Solvent is water Solution is Syrup Solute is Sugar
Answered by Doug =] - Sat Apr 12 07:55:44 2008
Q. a mixture of syrup is made by dissolving sugar in water in a beaker. identify the solvent, solution and solute solvent = solution = solute = thanks for you time and help x
Asked by . . .pInKii PoOpEr. . . - Sat Apr 12 06:44:08 2008 - - 4 Answers - 0 Comments
A. Solvent is water Solution is Syrup Solute is Sugar
Answered by Doug =] - Sat Apr 12 07:55:44 2008
When potassium nitrate, KNO3, is dissolved in water, why is energy absorbed?
Q. Shouldn't energy be released? Breaking KNO3 bonds requires energy, but desolving means new bonds are formed between the solvent and solute which releases energy. Isn't the net difference in energy positive?
Asked by mmm - Mon Jun 15 11:48:56 2009 - - 1 Answers - 0 Comments
Q. Shouldn't energy be released? Breaking KNO3 bonds requires energy, but desolving means new bonds are formed between the solvent and solute which releases energy. Isn't the net difference in energy positive?
Asked by mmm - Mon Jun 15 11:48:56 2009 - - 1 Answers - 0 Comments
When the solvent temperature increases why does the time taken to dissolve the solute increase?
Q. When the solvent temperature increases why does the time taken to dissolve the solute increase?
Asked by Angel Gigglez - Fri Apr 17 20:39:42 2009 - - 1 Answers - 0 Comments
A. This question doesn't make logical sense. As you heat the system, you can dissolve more solute. As the solute concentration begins to reach maximum concentration, the rate of dissolution slows down. So if I have two beakers of solvent, one at 20 C the other at 50 C, and I drop in 1 g of Solute 1, then it will absolutely dissolve faster in the warmer solvent. This is a direct result of kinetics - the warmer something is, the more molecular motions present, and the more collisions will occur between the solute and the solvent. I'm not sure what you were trying to ask, or if you were just mixed up, but there ya go.
Answered by Jess4352 - Fri Apr 17 22:04:37 2009
Q. When the solvent temperature increases why does the time taken to dissolve the solute increase?
Asked by Angel Gigglez - Fri Apr 17 20:39:42 2009 - - 1 Answers - 0 Comments
A. This question doesn't make logical sense. As you heat the system, you can dissolve more solute. As the solute concentration begins to reach maximum concentration, the rate of dissolution slows down. So if I have two beakers of solvent, one at 20 C the other at 50 C, and I drop in 1 g of Solute 1, then it will absolutely dissolve faster in the warmer solvent. This is a direct result of kinetics - the warmer something is, the more molecular motions present, and the more collisions will occur between the solute and the solvent. I'm not sure what you were trying to ask, or if you were just mixed up, but there ya go.
Answered by Jess4352 - Fri Apr 17 22:04:37 2009
A soultion with a large amount of solute dissolved in a solvent is_____? Same question but with Small amount?
Q. A soultion with a large amount of solute dissolved in a solvent is___? Same question but with Small amount?
Asked by Rakino - Thu Apr 2 16:48:55 2009 - - 1 Answers - 0 Comments
A. concentrated / dilute
Answered by unknown - Thu Apr 2 16:56:52 2009
Q. A soultion with a large amount of solute dissolved in a solvent is___? Same question but with Small amount?
Asked by Rakino - Thu Apr 2 16:48:55 2009 - - 1 Answers - 0 Comments
A. concentrated / dilute
Answered by unknown - Thu Apr 2 16:56:52 2009
Not all solutes dissolve when they are warmed. In addition to cerium sulfate, can you think of two others?!?!?
Q. I need to figure out two more solvents that don't dissolve better in warmer water!
Asked by Woinen - Mon Jan 5 20:31:17 2009 - - 2 Answers - 0 Comments
A. gas and noble gas
Answered by Golu S - Mon Jan 5 20:35:44 2009
Q. I need to figure out two more solvents that don't dissolve better in warmer water!
Asked by Woinen - Mon Jan 5 20:31:17 2009 - - 2 Answers - 0 Comments
A. gas and noble gas
Answered by Golu S - Mon Jan 5 20:35:44 2009
Why does a matter dissolve in another matter?
Q. I want to understand mechanism of solubility> I know "like dissolves like" i.e. polar substance will dissolve in polar and non-polar will dissolve in non-polar solvent. Can the solubility be predicted on the basis of probability of some kind of bond formation/interaction between solute and solvent?
Asked by Somnath Singh - Tue Aug 14 15:15:49 2007 - - 1 Answers - 0 Comments
A. It is a matter of electrical attraction. For example, when NaCl dissolves in H2O, the Na+ and Cl- ions dissociate The Na+ ions are atracted to the Oxygen end of the water molecule and the Cl- ions are attracted to the hydrogen end. This is what dissolving is all about.
Answered by reb1240 - Tue Aug 14 17:05:49 2007
Q. I want to understand mechanism of solubility> I know "like dissolves like" i.e. polar substance will dissolve in polar and non-polar will dissolve in non-polar solvent. Can the solubility be predicted on the basis of probability of some kind of bond formation/interaction between solute and solvent?
Asked by Somnath Singh - Tue Aug 14 15:15:49 2007 - - 1 Answers - 0 Comments
A. It is a matter of electrical attraction. For example, when NaCl dissolves in H2O, the Na+ and Cl- ions dissociate The Na+ ions are atracted to the Oxygen end of the water molecule and the Cl- ions are attracted to the hydrogen end. This is what dissolving is all about.
Answered by reb1240 - Tue Aug 14 17:05:49 2007
If something isnt completely dissolved (a solute in a solvent) will the freezing point depression...?
Q. be larger or smaller. I think that if the solid still exists in the solvent(water) than it will have a smaller freezing point depression but I'm not sure.
Asked by bobby_gurl_14 - Sun Sep 20 22:49:02 2009 - - 1 Answers - 0 Comments
Q. be larger or smaller. I think that if the solid still exists in the solvent(water) than it will have a smaller freezing point depression but I'm not sure.
Asked by bobby_gurl_14 - Sun Sep 20 22:49:02 2009 - - 1 Answers - 0 Comments
1. A mixture in which a solute is dissolved in a solvent is called a...?
Q. another question: 2. Two liquids that dissolve in each other are said to be...?
Asked by meganlynn2011 - Thu Mar 5 19:32:19 2009 - - 1 Answers - 0 Comments
Q. another question: 2. Two liquids that dissolve in each other are said to be...?
Asked by meganlynn2011 - Thu Mar 5 19:32:19 2009 - - 1 Answers - 0 Comments
molar concentration of a solution containing 4 mol of solute dissolved in 2L solvent is 2 mol/L true or false?
Q. is this true or false
Asked by A - Thu Aug 20 22:58:32 2009 - - 2 Answers - 0 Comments
A. 4mol / 2 L = 2 mol/L
Answered by RaZz - Thu Aug 20 23:56:53 2009
Q. is this true or false
Asked by A - Thu Aug 20 22:58:32 2009 - - 2 Answers - 0 Comments
A. 4mol / 2 L = 2 mol/L
Answered by RaZz - Thu Aug 20 23:56:53 2009
which of the following does not occur when a solid solute dissolves in a liquid solvent?
Q. A.attractions between the solute particles break B.intermolecular attractions between the solvent particles break C.attractions between the solute and the solvent particles remain static D.attractions between the solute and the solvent particles form
Asked by cria t - Mon Nov 17 09:36:27 2008 - - 1 Answers - 0 Comments
A. The answer is C.
Answered by Chem Tutor - Mon Nov 17 09:41:48 2008
Q. A.attractions between the solute particles break B.intermolecular attractions between the solvent particles break C.attractions between the solute and the solvent particles remain static D.attractions between the solute and the solvent particles form
Asked by cria t - Mon Nov 17 09:36:27 2008 - - 1 Answers - 0 Comments
A. The answer is C.
Answered by Chem Tutor - Mon Nov 17 09:41:48 2008
What combination of intermolecular forces will result in a solution where a large amount of solute dissolves?
Q. strong/weak solute-solute intermolecular forces and either strong/weak solute-solvent intermolecular forces? I think that its weak solute-solute and strong solute-solvent.
Asked by Allen - Sat Jul 4 12:14:49 2009 - - 1 Answers - 0 Comments
Q. strong/weak solute-solute intermolecular forces and either strong/weak solute-solvent intermolecular forces? I think that its weak solute-solute and strong solute-solvent.
Asked by Allen - Sat Jul 4 12:14:49 2009 - - 1 Answers - 0 Comments
The concentration of a solvent is the measurement of the amount of ?
Q. a. solvent dissolved in a fixed amount of the solution b. solute dissolved in a fixed amount of the solution c. solvent dissolved in a fixed amount of the solute
Asked by becca12694 - Sat Jan 31 14:27:34 2009 - - 1 Answers - 0 Comments
A. B
Answered by coops - Sat Jan 31 15:34:05 2009
Q. a. solvent dissolved in a fixed amount of the solution b. solute dissolved in a fixed amount of the solution c. solvent dissolved in a fixed amount of the solute
Asked by becca12694 - Sat Jan 31 14:27:34 2009 - - 1 Answers - 0 Comments
A. B
Answered by coops - Sat Jan 31 15:34:05 2009
A 0.832 m solution of the solute benzene dissolved in the solvent C4H8O is available. Calculate the mass ( kg?
Q. A 0.832 m solution of the solute benzene dissolved in the solvent C4H8O is available. Calculate the mass ( kg ) of the solution that must be taken to obtain 0.5307 kg of benzene. Molar Mass (g/mol): C6H6 78.11 C4H8O 72.12 Density ( kg/L ): C6H6 0.8786 C4H8O 0.8892 Name/Formula: benzene: C6H6 tetrahydrofuran: C4H8O
Asked by Lucy L - Sat Feb 21 16:19:58 2009 - - 1 Answers - 0 Comments
Q. A 0.832 m solution of the solute benzene dissolved in the solvent C4H8O is available. Calculate the mass ( kg ) of the solution that must be taken to obtain 0.5307 kg of benzene. Molar Mass (g/mol): C6H6 78.11 C4H8O 72.12 Density ( kg/L ): C6H6 0.8786 C4H8O 0.8892 Name/Formula: benzene: C6H6 tetrahydrofuran: C4H8O
Asked by Lucy L - Sat Feb 21 16:19:58 2009 - - 1 Answers - 0 Comments
Is the fact that water is the universal solvent a chemical or physical property of water?
Q. Dissolving is a physical property of matter, and since a solvent dissolves a solute, would that make being the universal solvent a physical property of water?
Asked by Mcubed - Sun Jul 26 17:28:25 2009 - - 3 Answers - 1 Comments
A. I would say "not really". Water is the "universal solvent" because it is cheap and common. "Physical Properties" generally denote things like changes of state, refraction, dielectric coefficient etc. Chemical properties deal with how water reacts to other substances. Calling water the "universal solvent" isn't defining a concrete property, so I wouldn't do that. In general though, it is fair to say that the ability to solvate a particular solute is a physical property. Just realize that water doesn't solvate everything, in fact it can be quite limited at times. ChemTeam is wrong. Check out the wikipedia entry on physical property. Solubility is listed as a property AND a physical property is defined as any change which does not… [cont.]
Answered by John H - Sun Jul 26 17:42:21 2009
Q. Dissolving is a physical property of matter, and since a solvent dissolves a solute, would that make being the universal solvent a physical property of water?
Asked by Mcubed - Sun Jul 26 17:28:25 2009 - - 3 Answers - 1 Comments
A. I would say "not really". Water is the "universal solvent" because it is cheap and common. "Physical Properties" generally denote things like changes of state, refraction, dielectric coefficient etc. Chemical properties deal with how water reacts to other substances. Calling water the "universal solvent" isn't defining a concrete property, so I wouldn't do that. In general though, it is fair to say that the ability to solvate a particular solute is a physical property. Just realize that water doesn't solvate everything, in fact it can be quite limited at times. ChemTeam is wrong. Check out the wikipedia entry on physical property. Solubility is listed as a property AND a physical property is defined as any change which does not… [cont.]
Answered by John H - Sun Jul 26 17:42:21 2009
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