Why is benzoic acid more attracted to methylene chloride, in terms of intermolecular forces?
Q. In a solvent extraction experiment the distribution ratio and percent extraction for benzoic acid in a methylene chloride/water solution. Based on the values obtained, which layer (methylene chloride or water) is the benzoic acid attracted to? How is this explained in terms of intermolecular forces?
Asked by philonious - Mon Jul 6 01:06:12 2009 - - 1 Answers - 0 Comments
A. The benzoic acid would be more attracted to the water molecules because both benzoic acid and water are very polarized molecules. While methylene chloride is polar, the strength of the chlorine molecules is not as strong as in water.
Answered by Hesacon - Mon Jul 6 01:52:51 2009
Q. In a solvent extraction experiment the distribution ratio and percent extraction for benzoic acid in a methylene chloride/water solution. Based on the values obtained, which layer (methylene chloride or water) is the benzoic acid attracted to? How is this explained in terms of intermolecular forces?
Asked by philonious - Mon Jul 6 01:06:12 2009 - - 1 Answers - 0 Comments
A. The benzoic acid would be more attracted to the water molecules because both benzoic acid and water are very polarized molecules. While methylene chloride is polar, the strength of the chlorine molecules is not as strong as in water.
Answered by Hesacon - Mon Jul 6 01:52:51 2009
What can you conclude about the state of the benzoic acid molecules?
Q. A solution of benzoic acid in benzene has a freezing point of 3.1oC and a boiling point of 82.6oC. The freezing point of pure benzene is 5.12oC and its boiling point is 80.1oC. What can you conclude about the state of the benzoic acid molecules at the two different sets of temperatures?
Asked by Goofing around for answers - Wed Sep 6 04:37:20 2006 - - 1 Answers - 0 Comments
A. There seems to be something wrong here a solute will lower the freezing point. Anyways fp depression and bp elevation are colligative properties - they depend on the number of solute molecules (size and mass are irrelevant). Benzoic acid is the classic example of a molecule that likes to dimerize in solution - probably more at lower temperatures. That is the point of the question - so work it out from there.
Answered by deflagrated - Wed Sep 6 07:27:45 2006
Q. A solution of benzoic acid in benzene has a freezing point of 3.1oC and a boiling point of 82.6oC. The freezing point of pure benzene is 5.12oC and its boiling point is 80.1oC. What can you conclude about the state of the benzoic acid molecules at the two different sets of temperatures?
Asked by Goofing around for answers - Wed Sep 6 04:37:20 2006 - - 1 Answers - 0 Comments
A. There seems to be something wrong here a solute will lower the freezing point. Anyways fp depression and bp elevation are colligative properties - they depend on the number of solute molecules (size and mass are irrelevant). Benzoic acid is the classic example of a molecule that likes to dimerize in solution - probably more at lower temperatures. That is the point of the question - so work it out from there.
Answered by deflagrated - Wed Sep 6 07:27:45 2006
When benzoic acid an quanine are dissolved in dichloromethane solution, will there be any other forms present?
Q. Benzoic acid pKa = 4.2 Quinine pKa = 8.5 The question actually says "besides the neutral forms of benzoic acid and quinine, will any other chemical form(s) be present" but I couldn't fit that in the box.
Asked by Rambler - Sun Aug 16 04:12:35 2009 - - 1 Answers - 0 Comments
A. Yes, there will be other forms present.
Answered by The Ugly Truth - Wed Aug 19 17:30:02 2009
Q. Benzoic acid pKa = 4.2 Quinine pKa = 8.5 The question actually says "besides the neutral forms of benzoic acid and quinine, will any other chemical form(s) be present" but I couldn't fit that in the box.
Asked by Rambler - Sun Aug 16 04:12:35 2009 - - 1 Answers - 0 Comments
A. Yes, there will be other forms present.
Answered by The Ugly Truth - Wed Aug 19 17:30:02 2009
What is the water solubility of benzoic acid?
Q. Problem: At 25 C, a saturated solution of benzoic acid (C6H5CO2H; Ka = 6.4 multiplied by 10-5) has a pH of 2.80. Calculate the water solubility of benzoic acid in moles per liter and grams per 100. milliliters.
Asked by Peter Parker - Tue Jun 9 17:12:58 2009 - - 1 Answers - 0 Comments
A. Benzoic acid dissociates according to: c h cooh c h coo + H with Ka = [C H COO ] [H ] / [C H COOH] Ignoring the small contribution of self ionization of water, all H is formed due to dissociation of benzoic acid. Therefore the concentration of H and benzoate ions are the same: [C H COO ] = [H ] = 10^-pH = 10^(-2.8) = 1.585 10 mol/L The concentration of undissociated benzoic acid equals total amount dissolved minus amount dissociated [C H COOH] = [C H COOH] - [C H COO ] = [C H COOH] - [H ] Hence: Ka = [H ] / ([C H COOH] - [H ]) So the total amount dissolved (= maximum soluble amount) is [C H COOH] = [H ] /Ka + [H ] = ([H ]/Ka - 1) [H ] = (1.585 10 ) /1.585 10 + 1.585 10 ) mol/L = (1.585 10 ) /1.585 10 + 1.585 10 ) [cont.]
Answered by schmiso - Wed Jun 10 17:03:52 2009
Q. Problem: At 25 C, a saturated solution of benzoic acid (C6H5CO2H; Ka = 6.4 multiplied by 10-5) has a pH of 2.80. Calculate the water solubility of benzoic acid in moles per liter and grams per 100. milliliters.
Asked by Peter Parker - Tue Jun 9 17:12:58 2009 - - 1 Answers - 0 Comments
A. Benzoic acid dissociates according to: c h cooh c h coo + H with Ka = [C H COO ] [H ] / [C H COOH] Ignoring the small contribution of self ionization of water, all H is formed due to dissociation of benzoic acid. Therefore the concentration of H and benzoate ions are the same: [C H COO ] = [H ] = 10^-pH = 10^(-2.8) = 1.585 10 mol/L The concentration of undissociated benzoic acid equals total amount dissolved minus amount dissociated [C H COOH] = [C H COOH] - [C H COO ] = [C H COOH] - [H ] Hence: Ka = [H ] / ([C H COOH] - [H ]) So the total amount dissolved (= maximum soluble amount) is [C H COOH] = [H ] /Ka + [H ] = ([H ]/Ka - 1) [H ] = (1.585 10 ) /1.585 10 + 1.585 10 ) mol/L = (1.585 10 ) /1.585 10 + 1.585 10 ) [cont.]
Answered by schmiso - Wed Jun 10 17:03:52 2009
What is the chemical equation for the ionization of benzoic acid?
Q. I'm working on acid/base chemistry...I'm stuck on this one...it asks to write the chemical equation, equilibrium constant expression and the value of the equilibrium constant for benzoic acid...help!? and guidance would be appreciated! Thanks!
Asked by Big T - Sat Mar 7 19:17:18 2009 - - 1 Answers - 0 Comments
A. Benzoic acid is an organic (carbon based) acid that can dissociate (lose its acidic proton) in water. Here is the equation... C6H5COOH --> C6H5COO(-) + H(+) The equilibrium constant for this dissociation is 6.3 X 10-5... Does this help? ;-)
Answered by David M - Sat Mar 7 20:34:18 2009
Q. I'm working on acid/base chemistry...I'm stuck on this one...it asks to write the chemical equation, equilibrium constant expression and the value of the equilibrium constant for benzoic acid...help!? and guidance would be appreciated! Thanks!
Asked by Big T - Sat Mar 7 19:17:18 2009 - - 1 Answers - 0 Comments
A. Benzoic acid is an organic (carbon based) acid that can dissociate (lose its acidic proton) in water. Here is the equation... C6H5COOH --> C6H5COO(-) + H(+) The equilibrium constant for this dissociation is 6.3 X 10-5... Does this help? ;-)
Answered by David M - Sat Mar 7 20:34:18 2009
How many moles of benzoic acid, a monoprotic acid with Ka=6.4 x 0^-5, must be dissolved in 500 mL of H2O to?
Q. How many moles of benzoic acid, a monoprotic acid with Ka=6.4 x 0^-5, must be dissolved in 500 mL of H2O to produce a solution with pH=2.50? Please show work!
Asked by Kiz - Mon Jul 6 16:04:47 2009 - - 0 Answers - 0 Comments
A. pH = -log[H+] = 2.5 [H+] = 3.162*10^-3 mol/litre Ka = [H+] * [A-] / [HA] = [H+]^2 / [HA] =6.4*10^-5 mol/litre [HA] = [H+]^2 / 6.4*10^-5 = 9.998*10^-6 / 6.4*10^-5 mol/litre = 0.156 mol/litre = 0.078 mol/ 500ml
Answered by jon - Mon Jul 6 16:39:12 2009
Q. How many moles of benzoic acid, a monoprotic acid with Ka=6.4 x 0^-5, must be dissolved in 500 mL of H2O to produce a solution with pH=2.50? Please show work!
Asked by Kiz - Mon Jul 6 16:04:47 2009 - - 0 Answers - 0 Comments
A. pH = -log[H+] = 2.5 [H+] = 3.162*10^-3 mol/litre Ka = [H+] * [A-] / [HA] = [H+]^2 / [HA] =6.4*10^-5 mol/litre [HA] = [H+]^2 / 6.4*10^-5 = 9.998*10^-6 / 6.4*10^-5 mol/litre = 0.156 mol/litre = 0.078 mol/ 500ml
Answered by jon - Mon Jul 6 16:39:12 2009
How would the freezing point depression of benzoic acid differ from sodum chloride?
Q. How would the freezing point depression of 1.0 molal aqueous solution of benzoic acid, (C6H5COOH) an organic compound, differ from that of a 1.0 molal aqueous solution of sodium chloride, NaCl, an ionic compound?? Hint: colligative properties, polar vs. nonpolar Also, if you could provide kf values to answer, this would be helpful. I can't find them anywhere.
Asked by zen_ohm - Fri Apr 4 22:52:03 2008 - - 3 Answers - 0 Comments
A. Benzoic acid is a weak acid and is essentially not dissociated, so the van't Hoff factor is really close to 1. The NaCl, on the other hand, dissociates completely into two particles, so the van't Hoff factor is almost 2. Since freezing point depression is a colligative property it depends only on "the collection of particles", and will be greater for the NaCl. delta T = (i)(kf)(m) were delta T is the difference in FP i is the van't Hoff factor kf is the freezing point depression constant for the solvent m is the molality
Answered by pisgahchemist - Fri Apr 4 23:05:17 2008
Q. How would the freezing point depression of 1.0 molal aqueous solution of benzoic acid, (C6H5COOH) an organic compound, differ from that of a 1.0 molal aqueous solution of sodium chloride, NaCl, an ionic compound?? Hint: colligative properties, polar vs. nonpolar Also, if you could provide kf values to answer, this would be helpful. I can't find them anywhere.
Asked by zen_ohm - Fri Apr 4 22:52:03 2008 - - 3 Answers - 0 Comments
A. Benzoic acid is a weak acid and is essentially not dissociated, so the van't Hoff factor is really close to 1. The NaCl, on the other hand, dissociates completely into two particles, so the van't Hoff factor is almost 2. Since freezing point depression is a colligative property it depends only on "the collection of particles", and will be greater for the NaCl. delta T = (i)(kf)(m) were delta T is the difference in FP i is the van't Hoff factor kf is the freezing point depression constant for the solvent m is the molality
Answered by pisgahchemist - Fri Apr 4 23:05:17 2008
How many grams of benzoic acid should be added?
Q. You prepare a buffer solution by dissolving 1.76 g each of benzoic acid, HC7H5O2, and sodium benzoate, NaC7H5O2, in 650.0 mL of water. pH of this is 4.13. how many grams of benzoic acid would be added to the 650 mL to reach a pH of 3.79? I'm not really sure of the process to figure this out. Thanks!
Asked by hotttiegrl9 - Thu Apr 3 20:13:53 2008 - - 1 Answers - 0 Comments
A. First, look for the molar masses: benzoic acid: 122.12 g/mol sodium benzoate: 144.11 g/mol Thus, 1.76 g of benzoic acid in 650.0 mL of water is: (1.76g)/(122.12 g/mol)/0.650L = (0.01441/0.650) M and 1.76 g of sodium benzoate in 650.0 mL of water is: (1.76g)/(144.11 g/mol)/0.650L = (0.01221/0.650) M Also, pH = 4.13 means [H+] = 10^-4.13 M. Hence: Ka = [C7H5O2-]*[H+]/[HC7H5O2] = 0.01221*10^-4.13/0.01441 = 6.281x10^-5 Now, to change to pH = 3.79 or [H+] = 10^-3.79M, we must have such benzoic acid concentration [HC7H5O2], that: Ka = 6.281x10^-5 = 0.01221*10^-3.79/([HC7H5O 2]*0.650) or: [HC7H5O2] = 0.01221*10^-3.79/(Ka*0.65 0) = (0.03153/0.650) M, which is (0.01711/0.650)M greater than what it was before. Thus the required mass of benzoic… [cont.]
Answered by Hahaha - Sun Apr 6 02:01:52 2008
Q. You prepare a buffer solution by dissolving 1.76 g each of benzoic acid, HC7H5O2, and sodium benzoate, NaC7H5O2, in 650.0 mL of water. pH of this is 4.13. how many grams of benzoic acid would be added to the 650 mL to reach a pH of 3.79? I'm not really sure of the process to figure this out. Thanks!
Asked by hotttiegrl9 - Thu Apr 3 20:13:53 2008 - - 1 Answers - 0 Comments
A. First, look for the molar masses: benzoic acid: 122.12 g/mol sodium benzoate: 144.11 g/mol Thus, 1.76 g of benzoic acid in 650.0 mL of water is: (1.76g)/(122.12 g/mol)/0.650L = (0.01441/0.650) M and 1.76 g of sodium benzoate in 650.0 mL of water is: (1.76g)/(144.11 g/mol)/0.650L = (0.01221/0.650) M Also, pH = 4.13 means [H+] = 10^-4.13 M. Hence: Ka = [C7H5O2-]*[H+]/[HC7H5O2] = 0.01221*10^-4.13/0.01441 = 6.281x10^-5 Now, to change to pH = 3.79 or [H+] = 10^-3.79M, we must have such benzoic acid concentration [HC7H5O2], that: Ka = 6.281x10^-5 = 0.01221*10^-3.79/([HC7H5O 2]*0.650) or: [HC7H5O2] = 0.01221*10^-3.79/(Ka*0.65 0) = (0.03153/0.650) M, which is (0.01711/0.650)M greater than what it was before. Thus the required mass of benzoic… [cont.]
Answered by Hahaha - Sun Apr 6 02:01:52 2008
Why is benzoic acid soluble in concentrated H2S04 but not soluble in 5% HCl?
Q. Isn't benzoic acid a weak acid? So why is it soluble in one strong acid and not in the other strong acid?
Asked by cool - Tue Nov 24 13:03:18 2009 - - 1 Answers - 0 Comments
A. Conc. H2SO4 is ~96% pure (only 4% water) while 5% HCl is only 5%.HCl and 95% water. Benzoic acid must not be soluble in the latter because of all of the water content. However, if 5% NaOH solution were used instead, the bezoic acid would be completely soluble since the carboxylic acid salt (sodium carboxylate) would form, which is water soluble... Hope this helps
Answered by David M - Tue Nov 24 13:11:40 2009
Q. Isn't benzoic acid a weak acid? So why is it soluble in one strong acid and not in the other strong acid?
Asked by cool - Tue Nov 24 13:03:18 2009 - - 1 Answers - 0 Comments
A. Conc. H2SO4 is ~96% pure (only 4% water) while 5% HCl is only 5%.HCl and 95% water. Benzoic acid must not be soluble in the latter because of all of the water content. However, if 5% NaOH solution were used instead, the bezoic acid would be completely soluble since the carboxylic acid salt (sodium carboxylate) would form, which is water soluble... Hope this helps
Answered by David M - Tue Nov 24 13:11:40 2009
How do you make benzoic acid from sodium benzoate?
Q. I think its sodium benzoate + hydronium --> benzoic acid + water but im not sure. Thanks!
Asked by Jamie_McFadden06 - Thu Jan 21 18:46:42 2010 - - 1 Answers - 0 Comments
A. yes
Answered by Steve O - Thu Jan 21 19:57:09 2010
Q. I think its sodium benzoate + hydronium --> benzoic acid + water but im not sure. Thanks!
Asked by Jamie_McFadden06 - Thu Jan 21 18:46:42 2010 - - 1 Answers - 0 Comments
A. yes
Answered by Steve O - Thu Jan 21 19:57:09 2010
When I added hydrochloric acid to benzoic acid, it oiled out. What should I do?
Q. When I added 6 M of hydrochloric acid to benzoic acid, there seemed to be a oil bubble and the pH of the liquid stayed at 6. What should I do to remove the oil bubble and how can I get benzoic acid crystals to form? Yes, the pH stayed at 6, which confuses me too because it should be at 3 or 2.
Asked by Maggie - Mon Nov 24 19:13:10 2008 - - 1 Answers - 0 Comments
A. Are you sure that "pH of the liquid stayed at 6"? I do not believe that the "adding hydrochloric acid to benzoic acid" would have pH as high as 6.
Answered by Hahaha - Mon Nov 24 20:50:25 2008
Q. When I added 6 M of hydrochloric acid to benzoic acid, there seemed to be a oil bubble and the pH of the liquid stayed at 6. What should I do to remove the oil bubble and how can I get benzoic acid crystals to form? Yes, the pH stayed at 6, which confuses me too because it should be at 3 or 2.
Asked by Maggie - Mon Nov 24 19:13:10 2008 - - 1 Answers - 0 Comments
A. Are you sure that "pH of the liquid stayed at 6"? I do not believe that the "adding hydrochloric acid to benzoic acid" would have pH as high as 6.
Answered by Hahaha - Mon Nov 24 20:50:25 2008
what are the reactions when benzoic acid and salicylic acid are mixed with soda lime?
Q. we had that experiment in chem class. we pulverized benzoic acid and soda lime. then we heated in a test tube. it smelled like paste and when i ignited the fumes going out of the tube yellow flame was produced. then with the salicylic acid i pulverized it with soda lime and when heated, smelled like paste too. then i added ferric chloride to the test tube and the resulting solution turned purple.
Asked by mit - Sat Jan 24 10:33:54 2009 - - 1 Answers - 1 Comments
A. I don't know. Did you try with Google ?
Answered by Etienne de Quercy, in God Mode - Wed Jan 28 09:20:55 2009
Q. we had that experiment in chem class. we pulverized benzoic acid and soda lime. then we heated in a test tube. it smelled like paste and when i ignited the fumes going out of the tube yellow flame was produced. then with the salicylic acid i pulverized it with soda lime and when heated, smelled like paste too. then i added ferric chloride to the test tube and the resulting solution turned purple.
Asked by mit - Sat Jan 24 10:33:54 2009 - - 1 Answers - 1 Comments
A. I don't know. Did you try with Google ?
Answered by Etienne de Quercy, in God Mode - Wed Jan 28 09:20:55 2009
Would decarboxylation occur when Benzoic acid, Sodium Carbonate and sand have Sulfurous acid added?
Q. I was wondering if anyone could tell me what would happen if Benzoic Acid, Sodium Carbonate and sand had Sulfurous acid added to it? Would there be any reactions that cause decarboxylation to occur? And would it occur at lower temperatures?
Asked by Jennifer C - Wed Apr 2 16:36:03 2008 - - 1 Answers - 0 Comments
A. No, there would be no reaction that would lead to decarboxylation of the acid group from the benzene ring with these reagent under any of these conditions. Ph-COOH(aq) + H2SO3(aq) + Na2CO3(aq) + sand --> Ph-COOH(aq) + Na2SO3(aq) + H2O(l) + CO2(g) + sand
Answered by Dr Dave P - Wed Apr 2 16:48:26 2008
Q. I was wondering if anyone could tell me what would happen if Benzoic Acid, Sodium Carbonate and sand had Sulfurous acid added to it? Would there be any reactions that cause decarboxylation to occur? And would it occur at lower temperatures?
Asked by Jennifer C - Wed Apr 2 16:36:03 2008 - - 1 Answers - 0 Comments
A. No, there would be no reaction that would lead to decarboxylation of the acid group from the benzene ring with these reagent under any of these conditions. Ph-COOH(aq) + H2SO3(aq) + Na2CO3(aq) + sand --> Ph-COOH(aq) + Na2SO3(aq) + H2O(l) + CO2(g) + sand
Answered by Dr Dave P - Wed Apr 2 16:48:26 2008
Why is Benzoic acid somewhat soluble in water?
Q. Why is Benzoic acid somewhat soluble in water?
Asked by M. G. - Fri Oct 2 10:50:03 2009 - - 1 Answers - 0 Comments
A. benzoic acid is nearly insoluble in cold water but sufficiently soluble in hot water ...this is because non-polar hydrocarbon part outweighs the effect of polar -COOH part as non polar part is hydrophobic ...so no hydrogen bonding takes place in cold water and it is insoluble... only aliphatic carboxylic acids having upto 4 carbon atoms are miscible in water due to the formation of hydrogen bonds but in hot water thermodynamics comes into play now as Gibbs energy is related to entropy change as (deltaG)=deltaH-T(deltaS) now as dissolution of benzoic acid crystal in water is an exothermic process so delta H is negative... now delta S is positive as solid is changing into liquid... so if we increase the temperature the overall gibb's… [cont.]
Answered by ashish sinha - Fri Oct 2 11:22:20 2009
Q. Why is Benzoic acid somewhat soluble in water?
Asked by M. G. - Fri Oct 2 10:50:03 2009 - - 1 Answers - 0 Comments
A. benzoic acid is nearly insoluble in cold water but sufficiently soluble in hot water ...this is because non-polar hydrocarbon part outweighs the effect of polar -COOH part as non polar part is hydrophobic ...so no hydrogen bonding takes place in cold water and it is insoluble... only aliphatic carboxylic acids having upto 4 carbon atoms are miscible in water due to the formation of hydrogen bonds but in hot water thermodynamics comes into play now as Gibbs energy is related to entropy change as (deltaG)=deltaH-T(deltaS) now as dissolution of benzoic acid crystal in water is an exothermic process so delta H is negative... now delta S is positive as solid is changing into liquid... so if we increase the temperature the overall gibb's… [cont.]
Answered by ashish sinha - Fri Oct 2 11:22:20 2009
what is the volume of water required to dissolve 1 g of benzoic acid at room temp?
Q. Also, what is the volume of boiling water needed to dissolve 1 g of benzoic acid? Question # 2 when is a mixture of solvents used to carry out a recrystallization instead of a single solvent?
Asked by Thomas B - Tue Oct 3 17:03:11 2006 - - 2 Answers - 0 Comments
A. The compound should be very soluble at the boiling point of the solvent and only sparingly soluble in the solvent at room temperature. This difference in solubility at hot versus cold temperatures is essential for the recrystallization process. If the compound is insoluble in the chosen solvent at high temperatures, then it will not dissolve. If the compound is very soluble in the solvent at room temperature, then getting the compound to crystallize in pure form from solution is difficult. For example, water is an excellent solvent for the recrystallization of benzoic acid. At 10 C only 2.1 g of benzoic acid dissolves in 1 liter of water, while at 95 C the solubility is 68 g/L.
Answered by Otts Shoals - Thu Oct 5 15:27:23 2006
Q. Also, what is the volume of boiling water needed to dissolve 1 g of benzoic acid? Question # 2 when is a mixture of solvents used to carry out a recrystallization instead of a single solvent?
Asked by Thomas B - Tue Oct 3 17:03:11 2006 - - 2 Answers - 0 Comments
A. The compound should be very soluble at the boiling point of the solvent and only sparingly soluble in the solvent at room temperature. This difference in solubility at hot versus cold temperatures is essential for the recrystallization process. If the compound is insoluble in the chosen solvent at high temperatures, then it will not dissolve. If the compound is very soluble in the solvent at room temperature, then getting the compound to crystallize in pure form from solution is difficult. For example, water is an excellent solvent for the recrystallization of benzoic acid. At 10 C only 2.1 g of benzoic acid dissolves in 1 liter of water, while at 95 C the solubility is 68 g/L.
Answered by Otts Shoals - Thu Oct 5 15:27:23 2006
Ether extraction of methyl benzoate and benzoic acid?
Q. A chemist has carried out a reaction to convert benzoic acid to methyl benzoate. Analysis of the crude product shows that there is about 10% of the starting benzoic acid present. Outline an ether extraction procedure that the chemist could carry out to remove the benzoic acid and isolate methyl benzoate.
Asked by Megiddo - Fri Jul 9 13:45:46 2010 - - 1 Answers - 0 Comments
A. Off the top of my head, I'd employ a base to separate the two. Benzoic acid is, well, an acid. As such, it'll react with a base and become benzoate, which is negatively charged. Charged species are soluble in water and other polar solvents, but nonpolar compounds are not. You can exploit this to flush out the benzoic acid. First, add to the mixture a moderately strong basic solution. This should convert all of the benzoic acid into benzoate, which will then dissolve readily in the aqueous base solution. Mix it around a bit to ensure that all the benzoic acid is dissolved, then let it settle until the aqueous layer and the organic layer are separated (they'll resemble oil and water, with a clear line between where the watery layer is and… [cont.]
Answered by Pye - Fri Jul 9 14:50:26 2010
Q. A chemist has carried out a reaction to convert benzoic acid to methyl benzoate. Analysis of the crude product shows that there is about 10% of the starting benzoic acid present. Outline an ether extraction procedure that the chemist could carry out to remove the benzoic acid and isolate methyl benzoate.
Asked by Megiddo - Fri Jul 9 13:45:46 2010 - - 1 Answers - 0 Comments
A. Off the top of my head, I'd employ a base to separate the two. Benzoic acid is, well, an acid. As such, it'll react with a base and become benzoate, which is negatively charged. Charged species are soluble in water and other polar solvents, but nonpolar compounds are not. You can exploit this to flush out the benzoic acid. First, add to the mixture a moderately strong basic solution. This should convert all of the benzoic acid into benzoate, which will then dissolve readily in the aqueous base solution. Mix it around a bit to ensure that all the benzoic acid is dissolved, then let it settle until the aqueous layer and the organic layer are separated (they'll resemble oil and water, with a clear line between where the watery layer is and… [cont.]
Answered by Pye - Fri Jul 9 14:50:26 2010
Why is benzoic acid used in some adhesives?
Q. What's so special about benzoic acid?
Asked by unknown - Sun Sep 6 12:00:47 2009 - - 1 Answers - 0 Comments
A. Lancenigo di Villorba (TV), Italy benzoic acid results the simplest organic acid. Looking for its molecular sketch ..H-C=C-H .../...\ H-C...C-COOH ...\\...// ..H-C--C-H it has the following characteristics : -) few polarity ; -) ionizable functional group. I hope this helps you.
Answered by Zor Prime - Sun Sep 6 12:10:30 2009
Q. What's so special about benzoic acid?
Asked by unknown - Sun Sep 6 12:00:47 2009 - - 1 Answers - 0 Comments
A. Lancenigo di Villorba (TV), Italy benzoic acid results the simplest organic acid. Looking for its molecular sketch ..H-C=C-H .../...\ H-C...C-COOH ...\\...// ..H-C--C-H it has the following characteristics : -) few polarity ; -) ionizable functional group. I hope this helps you.
Answered by Zor Prime - Sun Sep 6 12:10:30 2009
You are provided with stock solution of benzoic acid that has been prepared by dissolving 244mg of benzoic?
Q. acid in 1 dm^3 of ethyl acetate. You will need to calculate the concentration of this solution in mol.dm^3.. Also we have to calculate l of stock solution: 800 and l of ethyl acetate: 2200 and we have to find out the benzoic acid
Asked by Kat B - Sat Nov 24 10:02:42 2007 - - 1 Answers - 0 Comments
A. MW benzoic=122g/l 1mM =122/1000 or .122g/l .244g=2mM or .002Molar
Answered by natural-health-doctor.com - Sat Nov 24 10:27:32 2007
Q. acid in 1 dm^3 of ethyl acetate. You will need to calculate the concentration of this solution in mol.dm^3.. Also we have to calculate l of stock solution: 800 and l of ethyl acetate: 2200 and we have to find out the benzoic acid
Asked by Kat B - Sat Nov 24 10:02:42 2007 - - 1 Answers - 0 Comments
A. MW benzoic=122g/l 1mM =122/1000 or .122g/l .244g=2mM or .002Molar
Answered by natural-health-doctor.com - Sat Nov 24 10:27:32 2007
is it acetic acid and benzoic acid soluble in 5% NaHCO3 solution?
Q. The solubility of acetic and benzoic acid in 5% of naHCO3?
Asked by hannika - Mon Sep 3 07:33:35 2007 - - 2 Answers - 0 Comments
A. Both Acetic acid and Benzoic acid are soluble in 5 % Sodium Hydrogen Carbonate solution. CH3COOH (aq) + NaHCO3 (aq) --> CH3COONa (aq) + H2O (l) + CO2 (g) C6H5COOH (aq) + NaHCO3 (aq) --> C6H5COONa (aq) + H2O (l) + CO2 (g)
Answered by Richard - Mon Sep 3 07:49:06 2007
Q. The solubility of acetic and benzoic acid in 5% of naHCO3?
Asked by hannika - Mon Sep 3 07:33:35 2007 - - 2 Answers - 0 Comments
A. Both Acetic acid and Benzoic acid are soluble in 5 % Sodium Hydrogen Carbonate solution. CH3COOH (aq) + NaHCO3 (aq) --> CH3COONa (aq) + H2O (l) + CO2 (g) C6H5COOH (aq) + NaHCO3 (aq) --> C6H5COONa (aq) + H2O (l) + CO2 (g)
Answered by Richard - Mon Sep 3 07:49:06 2007
what is the difference between acetic acid and benzoic acid in cold water solubility?
Q. basically, why is acetic acid soluble in cold water while benzoic acid is not
Asked by t t - Wed Sep 26 21:33:43 2007 - - 2 Answers - 0 Comments
A. basically it comes down to size. As the molecular weight goes up the solubility goes down
Answered by Aurium - Wed Sep 26 21:44:24 2007
Q. basically, why is acetic acid soluble in cold water while benzoic acid is not
Asked by t t - Wed Sep 26 21:33:43 2007 - - 2 Answers - 0 Comments
A. basically it comes down to size. As the molecular weight goes up the solubility goes down
Answered by Aurium - Wed Sep 26 21:44:24 2007
From Yahoo Answer Search: 'benzoic acid'
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A Chinese red bun sample was found to contain the non-permitted colouring matter Rhodamine B while a nopal juice sample contained excessive benzoic acid and ...
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Dr. Eric
Sat, 26 Jun 2010 16:06:50 GM
Dimethicone, quaternium-18 hectorite, hydroxystearic acid, methicone, silk powder, SILICA, propylene carbonate, BHT, sorbic acid, methylparaben, propylparaben, topcoat contains: hydrogenated polydecene, SQUALANE, . benzoic acid. , ...
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