Solubility Answers
What are some patterns with regard to ions that tend to be of low solubility vs high solubility?
Q. I did a lab in AP Chemistry and we saw if certain reactions produced preecipitates or not. I had to write net ionic equations which I did. I need to know what some patterns are with regard to ions that tend to be of low solubility and those which tend to be of high solubility.
Asked by a Matica - Sun Nov 23 12:26:58 2008 - Chemistry - 1 Answers - Comments
A. Chloride and nitrate salts are soluble. Salts of higher valence cations (+2 or higher) are insoluble, unless they are chlorides or nitrates. Cations of +1 charge are soluble, except for silver. However, silver nitrate is soluble. Hydroxide salts of cations of +3 charge or higher are insoluble, except at low p H. Thus, for example, sodium chloride and silver nitrate are soluble, but if solutions are mixed, silver chloride precipitiates, leaving sodium nitrate in solution. Calcium nitrate mixed with sodium sulfate will precipitate calcium sulfate, leaving sodium nitrate in solution.
Answered by Glenguin - Mon Nov 24 08:55:25 2008
Q. I did a lab in AP Chemistry and we saw if certain reactions produced preecipitates or not. I had to write net ionic equations which I did. I need to know what some patterns are with regard to ions that tend to be of low solubility and those which tend to be of high solubility.
Asked by a Matica - Sun Nov 23 12:26:58 2008 - Chemistry - 1 Answers - Comments
A. Chloride and nitrate salts are soluble. Salts of higher valence cations (+2 or higher) are insoluble, unless they are chlorides or nitrates. Cations of +1 charge are soluble, except for silver. However, silver nitrate is soluble. Hydroxide salts of cations of +3 charge or higher are insoluble, except at low p H. Thus, for example, sodium chloride and silver nitrate are soluble, but if solutions are mixed, silver chloride precipitiates, leaving sodium nitrate in solution. Calcium nitrate mixed with sodium sulfate will precipitate calcium sulfate, leaving sodium nitrate in solution.
Answered by Glenguin - Mon Nov 24 08:55:25 2008
What is the trend in the solubility as the temperature is increased?
Q. What is the trend in the solubility as the temperature is increased?
Asked by - Fri Aug 20 17:21:22 2010 - Chemistry - 2 Answers - Comments
A. For most solids, the solubility increases as temperature increases. For dissolved gases, the solubility decreases as temperature increases. Look at the graph.
Answered by pisgahchemist - Fri Aug 20 17:36:22 2010
Q. What is the trend in the solubility as the temperature is increased?
Asked by - Fri Aug 20 17:21:22 2010 - Chemistry - 2 Answers - Comments
A. For most solids, the solubility increases as temperature increases. For dissolved gases, the solubility decreases as temperature increases. Look at the graph.
Answered by pisgahchemist - Fri Aug 20 17:36:22 2010
How do you use the solubility in order to predict the formation of a precipitate?
Q. How do you use the solubility in order to predict the formation of a precipitate like how do you use it to know what forms a precipitate? I already know that someone answered this already, but they didn't answer it very well...
Asked by - Wed Nov 18 02:19:31 2009 - Chemistry - 2 Answers - Comments
A. The answer to this question depends on the level to which you wish to go, and also the level of your understanding of chemistry. If you take a simple case: 25ml of 1.00 M solution of Na Cl is mixed with 25ml of 1.00M Ag NO3. Will a precipitate of Ag Cl form? Answer: Check a solubility table. Wikipedia is quite good, and derermine the solubility of Ag Cl: This is given as 520 I g/100 g at 50 A C. Now it does not take alot of knowledge to understand that you must have exceded this solubility and a precipitate will form. This is very easy answer to your question. The problem arises when you are dealing with extremely dilute solutions of solutes that can interreact to form a "possible" precipitate. This question of whether the… [cont.]
Answered by Trevor H - Wed Nov 18 04:50:11 2009
Q. How do you use the solubility in order to predict the formation of a precipitate like how do you use it to know what forms a precipitate? I already know that someone answered this already, but they didn't answer it very well...
Asked by - Wed Nov 18 02:19:31 2009 - Chemistry - 2 Answers - Comments
A. The answer to this question depends on the level to which you wish to go, and also the level of your understanding of chemistry. If you take a simple case: 25ml of 1.00 M solution of Na Cl is mixed with 25ml of 1.00M Ag NO3. Will a precipitate of Ag Cl form? Answer: Check a solubility table. Wikipedia is quite good, and derermine the solubility of Ag Cl: This is given as 520 I g/100 g at 50 A C. Now it does not take alot of knowledge to understand that you must have exceded this solubility and a precipitate will form. This is very easy answer to your question. The problem arises when you are dealing with extremely dilute solutions of solutes that can interreact to form a "possible" precipitate. This question of whether the… [cont.]
Answered by Trevor H - Wed Nov 18 04:50:11 2009
What factors happened to the ingredients to increase the rate of solubility? Were the ingredients, for exam?
Q. What factors happened to the ingredients to increase the rate of solubility? Were the ingredients, for example, stirred, heated, or added to help them dissolve?
Asked by - Tue Aug 10 16:06:39 2010 - Chemistry - 2 Answers - Comments
A. A lot depends on the ingredients. But lets say for the sake of argument that solubility was diffusion rate limited. In other words, if you just let it sit there, it would dissolve slowly since the concentration gradient changes very slowly. But stir it and the ingredients are always being exposed to a low level of similar ingredients, so it will dissolve faster. Heating will also work, as many things are more soluble in hot solution then cold, and also particles have more kinetic energy, and will diffuse faster.
Answered by cat lover - Tue Aug 10 16:19:51 2010
Q. What factors happened to the ingredients to increase the rate of solubility? Were the ingredients, for example, stirred, heated, or added to help them dissolve?
Asked by - Tue Aug 10 16:06:39 2010 - Chemistry - 2 Answers - Comments
A. A lot depends on the ingredients. But lets say for the sake of argument that solubility was diffusion rate limited. In other words, if you just let it sit there, it would dissolve slowly since the concentration gradient changes very slowly. But stir it and the ingredients are always being exposed to a low level of similar ingredients, so it will dissolve faster. Heating will also work, as many things are more soluble in hot solution then cold, and also particles have more kinetic energy, and will diffuse faster.
Answered by cat lover - Tue Aug 10 16:19:51 2010
How to determine the solubility of pure form of a drug sample ?
Q. If I have a drug sample that contain impurities,what would be a simple laboratory method to determine the solubility of the pure form of the drug ? I am seeking details of a method that uses solubilty phase diagram.
Asked by reenigne - Sat Dec 29 10:28:51 2007 - Chemistry - 1 Answers - Comments
A. If the suspected impurities are at all soluble, there is no way you can find out the solubility of the pure material, without purifying the drug. Any physical measurements you carry out are bound to refer to the mixture that you have.
Answered by Facts Matter - Sat Dec 29 12:04:55 2007
Q. If I have a drug sample that contain impurities,what would be a simple laboratory method to determine the solubility of the pure form of the drug ? I am seeking details of a method that uses solubilty phase diagram.
Asked by reenigne - Sat Dec 29 10:28:51 2007 - Chemistry - 1 Answers - Comments
A. If the suspected impurities are at all soluble, there is no way you can find out the solubility of the pure material, without purifying the drug. Any physical measurements you carry out are bound to refer to the mixture that you have.
Answered by Facts Matter - Sat Dec 29 12:04:55 2007
What is the relationship between the solubility rules?
Q. What is the relationship between the solubility rules in Table 4.1 and the list of strong bases in Table 4.2? Another way of asking this question is, why is Cd(OH)2, for example, not listed as a strong base?
Asked by Daylin Marie - Sun Sep 26 11:43:13 2010 - Chemistry - 1 Answers - Comments
A. Strong bases (and acids) are those which are completely ionised in aqueous solution. As Cd(OH)2 is not very soluble then it is only very slightly ionised in aqueous solution and so it is a weak base.
Answered by John - Sun Sep 26 11:46:46 2010
Q. What is the relationship between the solubility rules in Table 4.1 and the list of strong bases in Table 4.2? Another way of asking this question is, why is Cd(OH)2, for example, not listed as a strong base?
Asked by Daylin Marie - Sun Sep 26 11:43:13 2010 - Chemistry - 1 Answers - Comments
A. Strong bases (and acids) are those which are completely ionised in aqueous solution. As Cd(OH)2 is not very soluble then it is only very slightly ionised in aqueous solution and so it is a weak base.
Answered by John - Sun Sep 26 11:46:46 2010
What is the difference between solubility and dissolving?
Q. The rate of solubility and dissolving have different factors, but other than that, what's the difference between solubility and dissolving? This topic is coming out for my exams next week, and I'd really appreciate it if anyone who knows even a bit about this could help me out.
Asked by Hikari - Tue Aug 7 22:08:52 2007 - Chemistry - 1 Answers - Comments
A. Simplistically, solubility is the measure of how much "stuff" dissolves in a solvent. Dissolving is the physical action of one material (solute) moving into the solvent.
Answered by KennyB - Tue Aug 7 22:12:33 2007
Q. The rate of solubility and dissolving have different factors, but other than that, what's the difference between solubility and dissolving? This topic is coming out for my exams next week, and I'd really appreciate it if anyone who knows even a bit about this could help me out.
Asked by Hikari - Tue Aug 7 22:08:52 2007 - Chemistry - 1 Answers - Comments
A. Simplistically, solubility is the measure of how much "stuff" dissolves in a solvent. Dissolving is the physical action of one material (solute) moving into the solvent.
Answered by KennyB - Tue Aug 7 22:12:33 2007
How can we use solubility equations accurately when all materials are somewhat soluble?
Q. How can we use the theory of solubility and insolubility even though all materials are some what soluble. It seems that it may be generalizing to say that some materials are insoluble.
Asked by JDM89 - Tue Oct 28 02:51:41 2008 - Chemistry - 1 Answers - Comments
A. by measuring the solubility of the liquid
Answered by Justice C - Tue Oct 28 03:00:39 2008
Q. How can we use the theory of solubility and insolubility even though all materials are some what soluble. It seems that it may be generalizing to say that some materials are insoluble.
Asked by JDM89 - Tue Oct 28 02:51:41 2008 - Chemistry - 1 Answers - Comments
A. by measuring the solubility of the liquid
Answered by Justice C - Tue Oct 28 03:00:39 2008
What is the solubility of Magnesium Hydroxide in water?
Q. The solubility product constant of the magnesium hydroxide is 8.9 x 10^-12. Please explain your process and include a balaced equation if possible. Thanks.
Asked by kered628 - Tue May 29 18:34:16 2007 - Chemistry - 1 Answers - Comments
A. The reaction for the dissolution of Mg(OH)2 is: Mg(OH)2(s) = Mg++(aq) + 2OH-(aq) and the solubility product is: Ksp = AMg++A*AOH-A^2 = 8.9*10^-12 Each mole of Mg(OH)2 that dissolves produces one mole of Mg++ ions and two moles of OH- ions. If we let x be the concentration of Mg++ at equilibium, then by the stoichiometry of the reaction, AOH-A = 2*x We can then write the expression for the solubility product as: Ksp = x * (2x)^2 = 8.9*10^-12 Solving for x, 4x^3 = 8.9*10^-12 x^3 = 2.225*10^-12 x = 1.305*10^-4 This means that in a solution in equilibrium with solid Mg(OH)2, the concentration of Mg++ ions in solution will be 1.3*10^-4 M. To get this many moles of Mg++ ions in solution, an equal number of moles of Mg(OH)2 must dissolve, so the… [cont.]
Answered by hfshaw - Tue May 29 18:49:58 2007
Q. The solubility product constant of the magnesium hydroxide is 8.9 x 10^-12. Please explain your process and include a balaced equation if possible. Thanks.
Asked by kered628 - Tue May 29 18:34:16 2007 - Chemistry - 1 Answers - Comments
A. The reaction for the dissolution of Mg(OH)2 is: Mg(OH)2(s) = Mg++(aq) + 2OH-(aq) and the solubility product is: Ksp = AMg++A*AOH-A^2 = 8.9*10^-12 Each mole of Mg(OH)2 that dissolves produces one mole of Mg++ ions and two moles of OH- ions. If we let x be the concentration of Mg++ at equilibium, then by the stoichiometry of the reaction, AOH-A = 2*x We can then write the expression for the solubility product as: Ksp = x * (2x)^2 = 8.9*10^-12 Solving for x, 4x^3 = 8.9*10^-12 x^3 = 2.225*10^-12 x = 1.305*10^-4 This means that in a solution in equilibrium with solid Mg(OH)2, the concentration of Mg++ ions in solution will be 1.3*10^-4 M. To get this many moles of Mg++ ions in solution, an equal number of moles of Mg(OH)2 must dissolve, so the… [cont.]
Answered by hfshaw - Tue May 29 18:49:58 2007
What is the solubility of Na2SO4 in water at room temperature?
Q. And also, if you know, what is the solubility at room temp of these: Ca Cl2, Na Cl, Ca SO4 ? Thanks!
Asked by Cclizacf - Sun Feb 28 02:17:43 2010 - Chemistry - 1 Answers - Comments
A. 19.5 g of Na2SO4 in 100 g H2O @ 20 C 74.5 g of Ca Cl2 in 100 g H2O @ 20 C 35.9 g of Na Cl, in 100 g H2O @ 20 C 0.202 g of Ca SO4 in 100 g H2O @ 20 C (Ca SO4 was adapted from the solubility of Ca SO4*2H2O using a ratio of molar masses)
Answered by Steve O - Sun Feb 28 07:42:41 2010
Q. And also, if you know, what is the solubility at room temp of these: Ca Cl2, Na Cl, Ca SO4 ? Thanks!
Asked by Cclizacf - Sun Feb 28 02:17:43 2010 - Chemistry - 1 Answers - Comments
A. 19.5 g of Na2SO4 in 100 g H2O @ 20 C 74.5 g of Ca Cl2 in 100 g H2O @ 20 C 35.9 g of Na Cl, in 100 g H2O @ 20 C 0.202 g of Ca SO4 in 100 g H2O @ 20 C (Ca SO4 was adapted from the solubility of Ca SO4*2H2O using a ratio of molar masses)
Answered by Steve O - Sun Feb 28 07:42:41 2010
What is the solubility-prod uct constant for this salt at 25 degrees celsius?
Q. A 1.00 L solution saturated at 25 degrees celsius with lead (II) iodide contains 0.54 g of Pb I2. What is the solubility-prod uct constant for this salt at 25 degrees celsius? Please show how to do it.
Asked by thatonekid - Tue Dec 8 16:45:20 2009 - Chemistry - 1 Answers - Comments
A. moles Pb I2 = 0.54 g / 461.01 g/mol=0.0012 moles Pb2+ = 0.0012 moles I- = 2 x 0.0012 = 0.0024 Ksp = ( 0.0012)(0.0024) ^2=6.91 x 10^-9
Answered by Dr.A - Sat Dec 12 08:04:32 2009
Q. A 1.00 L solution saturated at 25 degrees celsius with lead (II) iodide contains 0.54 g of Pb I2. What is the solubility-prod uct constant for this salt at 25 degrees celsius? Please show how to do it.
Asked by thatonekid - Tue Dec 8 16:45:20 2009 - Chemistry - 1 Answers - Comments
A. moles Pb I2 = 0.54 g / 461.01 g/mol=0.0012 moles Pb2+ = 0.0012 moles I- = 2 x 0.0012 = 0.0024 Ksp = ( 0.0012)(0.0024) ^2=6.91 x 10^-9
Answered by Dr.A - Sat Dec 12 08:04:32 2009
How is the solubility of carbon dioxide gas related to the temperature of the beverage?
Q. A student carefully removes the cap from a chilled bottle of pop. The open top is coverd with a balloon that is secured with tape. When she shakes the botlle, the balloon fills with gas. This sequence is repeated with an adentical bottle of pop at room temperature. Which balloon will fill with the greatest amount of gas?How is the solubility of carbon dioxide gas related to the temperature of the beverage?
Asked by - N oD N N I . a - Wed Nov 15 18:14:07 2006 - Chemistry - 4 Answers - Comments
A. It'll cost you 2 balloons and 2 sodas to find out. Solubility almost always increases with temperature, but this rule doesn't work with most gases. In fact, in the case of carbon dioxide, it decreases. The bubbling that you see when you open a bottle is not an effect of the bottle warming to room temperature, though. Increased pressure also increases the solubility and this pressure is released upon removing the cap.
Answered by Bo Peep - Wed Nov 15 18:15:33 2006
Q. A student carefully removes the cap from a chilled bottle of pop. The open top is coverd with a balloon that is secured with tape. When she shakes the botlle, the balloon fills with gas. This sequence is repeated with an adentical bottle of pop at room temperature. Which balloon will fill with the greatest amount of gas?How is the solubility of carbon dioxide gas related to the temperature of the beverage?
Asked by - N oD N N I . a - Wed Nov 15 18:14:07 2006 - Chemistry - 4 Answers - Comments
A. It'll cost you 2 balloons and 2 sodas to find out. Solubility almost always increases with temperature, but this rule doesn't work with most gases. In fact, in the case of carbon dioxide, it decreases. The bubbling that you see when you open a bottle is not an effect of the bottle warming to room temperature, though. Increased pressure also increases the solubility and this pressure is released upon removing the cap.
Answered by Bo Peep - Wed Nov 15 18:15:33 2006
What is the solubility of CO2 in a soft drink that was bottled under a CO2 pressure of 4.5 atm?
Q. What is the solubility of CO2 in a soft drink (which is mainly water) that was bottled under a CO2 pressure of 4.5 atm? The solubility of CO2 gas in water is 0.15 g/100 m L at a pressure of 760 mm Hg?
Asked by Carmen - Sun Nov 15 23:20:35 2009 - Chemistry - 1 Answers - Comments
A. Henry's law says that concentration is proportional to pressure, p = kc. Increase the pressure by a factor of 4.5, increase the solubility by the same factor. 0.675 g/100 m L
Answered by im - Sun Nov 15 23:26:41 2009
Q. What is the solubility of CO2 in a soft drink (which is mainly water) that was bottled under a CO2 pressure of 4.5 atm? The solubility of CO2 gas in water is 0.15 g/100 m L at a pressure of 760 mm Hg?
Asked by Carmen - Sun Nov 15 23:20:35 2009 - Chemistry - 1 Answers - Comments
A. Henry's law says that concentration is proportional to pressure, p = kc. Increase the pressure by a factor of 4.5, increase the solubility by the same factor. 0.675 g/100 m L
Answered by im - Sun Nov 15 23:26:41 2009
Why is molecular weight and solubility an important tool for a scientist?
Q. please help me! why is knowing the molecular weight of a chemical an important tool for a scientist? and why is the solubility an important tool for a scientist?
Asked by Nancy - Sun Sep 26 22:33:38 2010 - Homework Help - 1 Answers - Comments
A. These are both basic properties that are easy to test when trying to analyze a material. Is this all you needed? If not, please post again.
Answered by norcekri - Mon Oct 4 19:37:53 2010
Q. please help me! why is knowing the molecular weight of a chemical an important tool for a scientist? and why is the solubility an important tool for a scientist?
Asked by Nancy - Sun Sep 26 22:33:38 2010 - Homework Help - 1 Answers - Comments
A. These are both basic properties that are easy to test when trying to analyze a material. Is this all you needed? If not, please post again.
Answered by norcekri - Mon Oct 4 19:37:53 2010
What does solubility have to do with chemical bonds?
Q. I have to write a paper on chemical bonds and i have to include solubility into it. I don't know how the 2 relate. Please explain
Asked by bronxbomber130 - Thu Oct 2 23:37:43 2008 - Chemistry - 1 Answers - Comments
A. Effect of chemical bonding on solubility Not all substances are equally soluble at the same temperature. At 41A F (5A C), the solubility of table sugar is more than three times greater than that of table salt, as shown in Figure 1. Even substances such as ordinary glass, which appear not to dissolve, actually do so, but their solubility values are extremely small. The types of bonds or forces that hold sugar particles together are different from those found in glass. The interaction between the attractive forces holding these particles together and the attractive forces to the molecules of solvents accounts for the different solubilities. Lou D'Amore
Answered by Shailu - Thu Oct 2 23:54:35 2008
Q. I have to write a paper on chemical bonds and i have to include solubility into it. I don't know how the 2 relate. Please explain
Asked by bronxbomber130 - Thu Oct 2 23:37:43 2008 - Chemistry - 1 Answers - Comments
A. Effect of chemical bonding on solubility Not all substances are equally soluble at the same temperature. At 41A F (5A C), the solubility of table sugar is more than three times greater than that of table salt, as shown in Figure 1. Even substances such as ordinary glass, which appear not to dissolve, actually do so, but their solubility values are extremely small. The types of bonds or forces that hold sugar particles together are different from those found in glass. The interaction between the attractive forces holding these particles together and the attractive forces to the molecules of solvents accounts for the different solubilities. Lou D'Amore
Answered by Shailu - Thu Oct 2 23:54:35 2008
How do you know whether a compound is soluble or its solubility in water?
Q. "write the firrmula of the following compounds and indicate its solubility in water" a) barium hydroxide d) barium sulfate j) potassium nitrate a is soluble d is insoluble and j insoluble, I know that because i have the answers, but why is that?
Asked by Iskandar - Tue Apr 22 03:36:31 2008 - Chemistry - 1 Answers - Comments
A. If you're in general chemistry, which I am assuming you are, you are simply supposed to follow the solubility rules (nitrates are always soluble, etc.) to determine which salts are soluble and which are not: Here's a more in depth answer:
Answered by derrp789 - Tue Apr 22 03:40:23 2008
Q. "write the firrmula of the following compounds and indicate its solubility in water" a) barium hydroxide d) barium sulfate j) potassium nitrate a is soluble d is insoluble and j insoluble, I know that because i have the answers, but why is that?
Asked by Iskandar - Tue Apr 22 03:36:31 2008 - Chemistry - 1 Answers - Comments
A. If you're in general chemistry, which I am assuming you are, you are simply supposed to follow the solubility rules (nitrates are always soluble, etc.) to determine which salts are soluble and which are not: Here's a more in depth answer:
Answered by derrp789 - Tue Apr 22 03:40:23 2008
How does increasing the water solubility of a drug molecule increase its chances of being excreted in the u?
Q. How does increasing the water solubility of a drug molecule increase its chances of being excreted in the urine?
Asked by barbie - Sun Oct 10 05:32:05 2010 - Medicine - 2 Answers - Comments
A. Think about it like this. Urine is primarily water - it's an aqueous phase of the body's chemistry. In order to eliminate a molecule in the urine, that molecule must be readily dissolvable in water. The more soluble a molecule is in water, the more can be dissolved into the urine. When designing drugs, this is an important challenge. Drugs must be water soluble enough to be absorbed by the body, since the stomach and intestines are aqueus phases. It also must have an amount of lipid solubility, to cross cell membranes, enter the brain, or another body compartment where the drug needs to be in order to work. Lipid and water solubility tend to be somewhat opposed to each other - molecules that dissolve well in one, do not dissolve well in… [cont.]
Answered by Az R - Sun Oct 10 06:58:29 2010
Q. How does increasing the water solubility of a drug molecule increase its chances of being excreted in the urine?
Asked by barbie - Sun Oct 10 05:32:05 2010 - Medicine - 2 Answers - Comments
A. Think about it like this. Urine is primarily water - it's an aqueous phase of the body's chemistry. In order to eliminate a molecule in the urine, that molecule must be readily dissolvable in water. The more soluble a molecule is in water, the more can be dissolved into the urine. When designing drugs, this is an important challenge. Drugs must be water soluble enough to be absorbed by the body, since the stomach and intestines are aqueus phases. It also must have an amount of lipid solubility, to cross cell membranes, enter the brain, or another body compartment where the drug needs to be in order to work. Lipid and water solubility tend to be somewhat opposed to each other - molecules that dissolve well in one, do not dissolve well in… [cont.]
Answered by Az R - Sun Oct 10 06:58:29 2010
solubility?
Q. when determining the solubility of a substance, why is it so important to stir the solution?
Asked by anita - Wed Jun 27 10:43:26 2007 - Chemistry - 4 Answers - Comments
A. Agitation (stirring) while dissolving a solid greatly accelerates dissolution rate and allows you to arrive at a saturated solution more efficiently and reliably. Without agitation, you will have to wait hours, perhaps days, for a saturated solution to develop on its own.
Answered by nardhelain - Wed Jun 27 12:17:32 2007
Q. when determining the solubility of a substance, why is it so important to stir the solution?
Asked by anita - Wed Jun 27 10:43:26 2007 - Chemistry - 4 Answers - Comments
A. Agitation (stirring) while dissolving a solid greatly accelerates dissolution rate and allows you to arrive at a saturated solution more efficiently and reliably. Without agitation, you will have to wait hours, perhaps days, for a saturated solution to develop on its own.
Answered by nardhelain - Wed Jun 27 12:17:32 2007
The ratio of solubility of compound A in benzene and water is 3. How many extractions with 50 ml of benzene ar?
Q. The ratio of solubility of compound A in benzene and water is 3. How many extractions with 50 ml of benzene are necessary to remove 80% of compound A from 100 ml of water solution?
Asked by stcong3 - Fri Jun 10 03:23:37 2011 - Chemistry - 1 Answers - Comments
A. 2. ratio is 3:1 or 75% to 25% first extraction, 75% of it is in benzene, 25% is in water second extraction, 81.25% of it is in benzene, 18.75% is in water. volume of aqueous or organic phase does not matter since its done in percentages, unless you use such as small amount that the solutes become saturated in the solvent.
Answered by K - Fri Jun 10 03:54:03 2011
Q. The ratio of solubility of compound A in benzene and water is 3. How many extractions with 50 ml of benzene are necessary to remove 80% of compound A from 100 ml of water solution?
Asked by stcong3 - Fri Jun 10 03:23:37 2011 - Chemistry - 1 Answers - Comments
A. 2. ratio is 3:1 or 75% to 25% first extraction, 75% of it is in benzene, 25% is in water second extraction, 81.25% of it is in benzene, 18.75% is in water. volume of aqueous or organic phase does not matter since its done in percentages, unless you use such as small amount that the solutes become saturated in the solvent.
Answered by K - Fri Jun 10 03:54:03 2011
How to calculate the solubility of a compound?
Q. I would like to know how to calculate the solubility of a compound in general and also have a specific question: The solubility of lead sulphate in water at 25 degrees C is 20.0 mg.dm-3. Wat is its solubility (in mg.dm-3) in 0.01 M Na2SO4 solution?
Asked by earthchild - Thu Jun 11 14:34:19 2009 - Chemistry - 4 Answers - Comments
A. for a sparingly soluble salt the Ksp is derived by assuming a small amount will dissolve and yield ions according to its composition.The small amount that dissolves IS the actual solubility of the salt in moles/L.. soo since you have a value of 20 mg/L as the solubility of Pb SO4 convert that to moles /L by dividing the grams of Pb SO4/L (20 mg/L = 0.02 grams/L ) by the molar mass of Pb SO4 ( 207.2 + 32 + 64 = 303.2 grams/mole ) soo 0.02 grams /L / 303.2 grams/mol = 6.6 x 10^-5 moles/L = 6.6 X 10^-5 M as the actual solubility of Pb SO4 Setting this in the Ksp relationship Ksp( Pb SO4) = APb+2AASO4^-2A a small amount of the insoluble salt ( 6.6 X 10^-5 M ) dissolved to yield 6.6 X 10^-5 M Pb+2 AND 6.6 X 10^-5 M SO4^-2 soo the Ksp =… [cont.]
Answered by Merlin's Feline - Thu Jun 11 15:17:47 2009
Q. I would like to know how to calculate the solubility of a compound in general and also have a specific question: The solubility of lead sulphate in water at 25 degrees C is 20.0 mg.dm-3. Wat is its solubility (in mg.dm-3) in 0.01 M Na2SO4 solution?
Asked by earthchild - Thu Jun 11 14:34:19 2009 - Chemistry - 4 Answers - Comments
A. for a sparingly soluble salt the Ksp is derived by assuming a small amount will dissolve and yield ions according to its composition.The small amount that dissolves IS the actual solubility of the salt in moles/L.. soo since you have a value of 20 mg/L as the solubility of Pb SO4 convert that to moles /L by dividing the grams of Pb SO4/L (20 mg/L = 0.02 grams/L ) by the molar mass of Pb SO4 ( 207.2 + 32 + 64 = 303.2 grams/mole ) soo 0.02 grams /L / 303.2 grams/mol = 6.6 x 10^-5 moles/L = 6.6 X 10^-5 M as the actual solubility of Pb SO4 Setting this in the Ksp relationship Ksp( Pb SO4) = APb+2AASO4^-2A a small amount of the insoluble salt ( 6.6 X 10^-5 M ) dissolved to yield 6.6 X 10^-5 M Pb+2 AND 6.6 X 10^-5 M SO4^-2 soo the Ksp =… [cont.]
Answered by Merlin's Feline - Thu Jun 11 15:17:47 2009
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Q: How can the p H and solubility show the difference between fumaric acid and maleic acid ... Consider the solubility equilibrium of calcium hydroxide, Ca(OH)2: ...
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Solubility is the property of a solid, liquid, or gaseous chemical substance called solute to dissolve in a solid, liquid, or gaseous solvent to form a homogeneous solution of the solute in the solvent. The solubility of a substance fundamentally depends on the used solvent as well as on temperature and pressure. The extent of the solubility of a substance in a specific solvent is measured as the saturation concentration where adding more solute does not increase the concentration of the solution.
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