If oxalic acid is a poison, why is it possible to eat rhubarb and spinach?
Q. Oxalic acid is used in wood bleaching agents and rust removers. How can we eat it? It is in spinach and rhubarb. Please answer! Thanks.
Asked by ???? - Wed Apr 18 05:31:39 2007 - - 3 Answers - 0 Comments
A. Look, every poison has its own fatal dose. Oxalic acid is is indeed a poison & its fatal dose is 5-15 (22 gm according to some) gm.Rhubarb contains the highest content of oxalic acid ( about 0.3-1.5 gms per 100 gm) & spinach contains 0.32-1.26 gms per 100 gm. This means that if one has to die by oxalic acid poisoning, he/she has to consume 100x10 = 1 kg of rhubarb or nearly 2 kgs of spinach at once. Imagine the sequence, one is intaking 1 kg of veggie at a time, also because of our cooking process the oxallic acid concentrations in those vegs decrease, which makes the fatal dose of such vegs still more higher & almost inpracticable. That is why, although oxallic acid is a poison, one do not dies by eating spinach or rhuharb.
Answered by s0u1 reaver - Wed Apr 18 06:10:11 2007
Q. Oxalic acid is used in wood bleaching agents and rust removers. How can we eat it? It is in spinach and rhubarb. Please answer! Thanks.
Asked by ???? - Wed Apr 18 05:31:39 2007 - - 3 Answers - 0 Comments
A. Look, every poison has its own fatal dose. Oxalic acid is is indeed a poison & its fatal dose is 5-15 (22 gm according to some) gm.Rhubarb contains the highest content of oxalic acid ( about 0.3-1.5 gms per 100 gm) & spinach contains 0.32-1.26 gms per 100 gm. This means that if one has to die by oxalic acid poisoning, he/she has to consume 100x10 = 1 kg of rhubarb or nearly 2 kgs of spinach at once. Imagine the sequence, one is intaking 1 kg of veggie at a time, also because of our cooking process the oxallic acid concentrations in those vegs decrease, which makes the fatal dose of such vegs still more higher & almost inpracticable. That is why, although oxallic acid is a poison, one do not dies by eating spinach or rhuharb.
Answered by s0u1 reaver - Wed Apr 18 06:10:11 2007
How do I use oxalic acid to whiten when I laundry our white clothes?
Q. Someone has told me that oxalic acid helps maintaining white clothes when used during laundry but didn't elaborate how to use it. Anybody knows how?
Asked by jinx - Sun Apr 13 09:46:41 2008 - - 1 Answers - 0 Comments
A. If you are trying to remove perspiration stains then I would suggest OxyMagic or some other oxygen compound instead of oxalic. Oxalic acid is stronger than vinegar and can cause some additional problems in the laundry. The cleaners that are Oxy-this-that-or-the-othe r are alkaline cleaners and should lift the stains more easily. Make sure that you are not adding dark or colored items to the whites, these items will bleed and can leave a dingy coloration on the clothes. You might even try the dye trap cloths in the laundry aisle. Shout has one called Color Catcher. I found the microfiber cloths I used for dusting did the same thing. The brilliant yellow came out dingy when washed with other items and the colors were ones I didn't… [cont.]
Answered by Dirk H - Mon Apr 14 23:15:45 2008
Q. Someone has told me that oxalic acid helps maintaining white clothes when used during laundry but didn't elaborate how to use it. Anybody knows how?
Asked by jinx - Sun Apr 13 09:46:41 2008 - - 1 Answers - 0 Comments
A. If you are trying to remove perspiration stains then I would suggest OxyMagic or some other oxygen compound instead of oxalic. Oxalic acid is stronger than vinegar and can cause some additional problems in the laundry. The cleaners that are Oxy-this-that-or-the-othe r are alkaline cleaners and should lift the stains more easily. Make sure that you are not adding dark or colored items to the whites, these items will bleed and can leave a dingy coloration on the clothes. You might even try the dye trap cloths in the laundry aisle. Shout has one called Color Catcher. I found the microfiber cloths I used for dusting did the same thing. The brilliant yellow came out dingy when washed with other items and the colors were ones I didn't… [cont.]
Answered by Dirk H - Mon Apr 14 23:15:45 2008
What is the percentage composition of oxalic acid?
Q. I have a chemistry question that asks: Find the percentage composition by mass of oxalic acid H2C2O4.2H2O Just need a bit of help with it and would like it shown with working out. Thanks :)
Asked by Aishy - Sat Dec 13 23:36:23 2008 - - 1 Answers - 0 Comments
A. molar mass = 126.07 g/mol % C = 2 x 12.011 x 100 / 126.07 = 19.1 % H = 6 x 1.008 x 100 / 126.07 = 4.80 % O = 6 x 15.9994 x 100 / 126.07 = 76.1
Answered by Dr.A - Sun Dec 14 08:22:11 2008
Q. I have a chemistry question that asks: Find the percentage composition by mass of oxalic acid H2C2O4.2H2O Just need a bit of help with it and would like it shown with working out. Thanks :)
Asked by Aishy - Sat Dec 13 23:36:23 2008 - - 1 Answers - 0 Comments
A. molar mass = 126.07 g/mol % C = 2 x 12.011 x 100 / 126.07 = 19.1 % H = 6 x 1.008 x 100 / 126.07 = 4.80 % O = 6 x 15.9994 x 100 / 126.07 = 76.1
Answered by Dr.A - Sun Dec 14 08:22:11 2008
How do u figure these kinda questions out? Oxalic acid is a diprotic acid. Calculate the weight of oxalic?
Q. Oxalic acid is a diprotic acid. Calculate the weight of oxalic acid, (COOH)2, molar mass = 90.04 g mol 1, in a sample that required 34.56 mL of 0.2345 M NaOH solution for complete neutralization.
Asked by S N - Mon Jul 14 07:17:44 2008 - - 1 Answers - 0 Comments
A. You figure them out by first looking at the equation that shows how the compounds interact. In this case, since oxalic acid (OA) is diprotic, one mole of OA will require 2 moles of NaOH. So you have OA + 2 NaOH ==> 2NaOxalate + H2O Now, how many moles of NaOH were used? It would be 0.3456 L x 0.2345 mol/L = 0.081 moles. Thus, there must be 1/2 that many moles of OA or 0.04 moles of OA. Molar mass of OA is 90.04 gm/mole x 0.04 moles = 3.6 gms.
Answered by Simonizer1218 - Mon Jul 14 07:35:51 2008
Q. Oxalic acid is a diprotic acid. Calculate the weight of oxalic acid, (COOH)2, molar mass = 90.04 g mol 1, in a sample that required 34.56 mL of 0.2345 M NaOH solution for complete neutralization.
Asked by S N - Mon Jul 14 07:17:44 2008 - - 1 Answers - 0 Comments
A. You figure them out by first looking at the equation that shows how the compounds interact. In this case, since oxalic acid (OA) is diprotic, one mole of OA will require 2 moles of NaOH. So you have OA + 2 NaOH ==> 2NaOxalate + H2O Now, how many moles of NaOH were used? It would be 0.3456 L x 0.2345 mol/L = 0.081 moles. Thus, there must be 1/2 that many moles of OA or 0.04 moles of OA. Molar mass of OA is 90.04 gm/mole x 0.04 moles = 3.6 gms.
Answered by Simonizer1218 - Mon Jul 14 07:35:51 2008
Can anybody tell me the reaction equation between oxalic acid and potassium permanganate?
Q. Its used in an experiment about adsorptionmof oxalic acid using acitivated charcoal and its really important!
Asked by meg_dcu - Sun Mar 4 18:13:35 2007 - - 1 Answers - 0 Comments
A. 2(MnO4)- + 5C2O4H2 + 6H+ ---> 2Mn2+ + 10CO2 + 8H2O
Answered by Gervald F - Sun Mar 4 18:19:12 2007
Q. Its used in an experiment about adsorptionmof oxalic acid using acitivated charcoal and its really important!
Asked by meg_dcu - Sun Mar 4 18:13:35 2007 - - 1 Answers - 0 Comments
A. 2(MnO4)- + 5C2O4H2 + 6H+ ---> 2Mn2+ + 10CO2 + 8H2O
Answered by Gervald F - Sun Mar 4 18:19:12 2007
Where can I buy Oxalic acid?
Q. I live in Dade City, Florida. I am looking for oxalic acid to make a rust removing bath for some engine parts. I am not sure where to find it though. I have looked at Lowes and did not find it. Where else can I look, I don't want to buy online and have it shipped.
Asked by Brandon H. - Thu Mar 5 23:58:17 2009 - - 2 Answers - 0 Comments
A. I believe that you can find it at an auto parts store like NAPA, Checker, etc. It should be sold as a radiator cleaner and is a crystalline product.
Answered by rofe - Fri Mar 6 00:11:55 2009
Q. I live in Dade City, Florida. I am looking for oxalic acid to make a rust removing bath for some engine parts. I am not sure where to find it though. I have looked at Lowes and did not find it. Where else can I look, I don't want to buy online and have it shipped.
Asked by Brandon H. - Thu Mar 5 23:58:17 2009 - - 2 Answers - 0 Comments
A. I believe that you can find it at an auto parts store like NAPA, Checker, etc. It should be sold as a radiator cleaner and is a crystalline product.
Answered by rofe - Fri Mar 6 00:11:55 2009
the combustion of 90 g of oxalic acid C2H2O4 in a bomb calometer whose?
Q. the combustion of 90 g of oxalic acid C2H2O4 in a bomb calometer whose heat capacity is 4.60 kj/Celcius causes the temperature to rise from 25 celcius to 79.6 celcius. what is the heat of combustion of oxalic acid
Asked by shazad b - Tue Apr 14 09:04:44 2009 - - 1 Answers - 0 Comments
Q. the combustion of 90 g of oxalic acid C2H2O4 in a bomb calometer whose heat capacity is 4.60 kj/Celcius causes the temperature to rise from 25 celcius to 79.6 celcius. what is the heat of combustion of oxalic acid
Asked by shazad b - Tue Apr 14 09:04:44 2009 - - 1 Answers - 0 Comments
In the UK, where can I buy Oxalic Acid to remove rust?
Q. I need to remove some rust. Ive tried White wine vinegar and baking powder but not doing a great job. Oxalic Acid should do the job Any ideas?
Asked by Doggy - Thu Feb 12 08:00:12 2009 - - 4 Answers - 0 Comments
Q. I need to remove some rust. Ive tried White wine vinegar and baking powder but not doing a great job. Oxalic Acid should do the job Any ideas?
Asked by Doggy - Thu Feb 12 08:00:12 2009 - - 4 Answers - 0 Comments
What is the gram molecular mass of oxalic acid?
Q. formula: H2C2O4-2H2O the little dash thing means with or soemthing i got 126.08 g/mole, but im not sure if i did this right could someone explain how to find this and if my answer is okay? thanks!
Asked by natty s - Tue May 27 20:24:17 2008 - - 1 Answers - 0 Comments
A. 126.08 is correct the little dash is really a dot. I call it a sticky dot. It connects the oxalic acid to the water. Oxalic acid is a hydrated compound, which means it has water as part of its structure.
Answered by zippythewonderslugohio - Tue May 27 20:31:53 2008
Q. formula: H2C2O4-2H2O the little dash thing means with or soemthing i got 126.08 g/mole, but im not sure if i did this right could someone explain how to find this and if my answer is okay? thanks!
Asked by natty s - Tue May 27 20:24:17 2008 - - 1 Answers - 0 Comments
A. 126.08 is correct the little dash is really a dot. I call it a sticky dot. It connects the oxalic acid to the water. Oxalic acid is a hydrated compound, which means it has water as part of its structure.
Answered by zippythewonderslugohio - Tue May 27 20:31:53 2008
Help with Titration of Oxalic Acid with Permanganate problem?
Q. What volume of 0.01980 M KMnO4 solution is required to titrate 25.00 mL of 0.06120 M H2C2O4, in acid solution?
Asked by Dan W - Fri Oct 10 13:00:21 2008 - - 1 Answers - 0 Comments
A. 2 MnO4- + 5 H2C2O4 + 6 H+ >> 2 Mn2+ + 10 CO2 + 8 H2O Moles oxalic acid = 0.02500 L x 0.06120 = 0.01530 Moles MnO4- = 0.01530 x 2 / 5 = 0.000612 V = 0.000612 / 0.01980 = 0.03091 L => 30.91 mL
Answered by Dr.A - Fri Oct 10 14:52:04 2008
Q. What volume of 0.01980 M KMnO4 solution is required to titrate 25.00 mL of 0.06120 M H2C2O4, in acid solution?
Asked by Dan W - Fri Oct 10 13:00:21 2008 - - 1 Answers - 0 Comments
A. 2 MnO4- + 5 H2C2O4 + 6 H+ >> 2 Mn2+ + 10 CO2 + 8 H2O Moles oxalic acid = 0.02500 L x 0.06120 = 0.01530 Moles MnO4- = 0.01530 x 2 / 5 = 0.000612 V = 0.000612 / 0.01980 = 0.03091 L => 30.91 mL
Answered by Dr.A - Fri Oct 10 14:52:04 2008
Potassium Permanganate and Oxalic acid titration?
Q. why doe we add sulfuric acid to the oxalic acid solution and then boil it? also what removes permanganate stains from skin?
Asked by Syl S - Mon Jan 12 13:56:16 2009 - - 1 Answers - 1 Comments
A. This is a redox titration where oxalic acid is oxidised to carbon dioxide: H2C2O4 ---> 2CO2 + 2H+ + 2e- and permanganate ions are reduced to manganese(II): (MnO4)- + 8H+ + 5e- ---> Mn2+ + 4H2O for an overall reaction of: 5 H2C2O4 + 2 (MnO4)- + 6 H+ ---> 10 CO2 + 2 Mn2+ + 8H2O For this reaction to occur, we need oxalic acid, permanganate ions, and a source of protons. The sulfuric acid is the source of protons. As for the stains, they are manganese(IV) oxide, MnO2, and they wear off with time.
Answered by JayJay - Mon Jan 12 14:41:40 2009
Q. why doe we add sulfuric acid to the oxalic acid solution and then boil it? also what removes permanganate stains from skin?
Asked by Syl S - Mon Jan 12 13:56:16 2009 - - 1 Answers - 1 Comments
A. This is a redox titration where oxalic acid is oxidised to carbon dioxide: H2C2O4 ---> 2CO2 + 2H+ + 2e- and permanganate ions are reduced to manganese(II): (MnO4)- + 8H+ + 5e- ---> Mn2+ + 4H2O for an overall reaction of: 5 H2C2O4 + 2 (MnO4)- + 6 H+ ---> 10 CO2 + 2 Mn2+ + 8H2O For this reaction to occur, we need oxalic acid, permanganate ions, and a source of protons. The sulfuric acid is the source of protons. As for the stains, they are manganese(IV) oxide, MnO2, and they wear off with time.
Answered by JayJay - Mon Jan 12 14:41:40 2009
what is the use of sulphuric acid in the reaction between oxalic acid and potassium permanganate?
Q. i just know it is to acidify the solution but can you explain in detail thanks i know it is to acidfy the sulotion but i need detail explanation also what is the purpose for heating the oxalic acid solution b4 titrating??
Asked by kev - Tue Aug 21 02:59:17 2007 - - 2 Answers - 0 Comments
A. The (MnO4)- ion needs H+ ions in order to take away the O atoms to make water - look at the half-equation: (MnO4)- + 8H+ + 5e- ---> Mn2+ + 4H2O The reaction is heated in order to speed up the reaction, which is very slow at room temperature.
Answered by Gervald F - Tue Aug 21 03:10:34 2007
Q. i just know it is to acidify the solution but can you explain in detail thanks i know it is to acidfy the sulotion but i need detail explanation also what is the purpose for heating the oxalic acid solution b4 titrating??
Asked by kev - Tue Aug 21 02:59:17 2007 - - 2 Answers - 0 Comments
A. The (MnO4)- ion needs H+ ions in order to take away the O atoms to make water - look at the half-equation: (MnO4)- + 8H+ + 5e- ---> Mn2+ + 4H2O The reaction is heated in order to speed up the reaction, which is very slow at room temperature.
Answered by Gervald F - Tue Aug 21 03:10:34 2007
Using just oxalic acid and distilled water, I wish to create a stock solution that is of pH 3....?
Q. How can I do this, knowing that the pKa of Oxalic acid is 1.27, and the volume of solution I wish to create is 200 ml or 0.2 L? Any help would be appreciated, thanks :)
Asked by TheBiochemist - Sun Mar 8 12:42:42 2009 - - 1 Answers - 0 Comments
A. Ka = [H+] [A-] / [HA] Since pH = 3, then [H+] = [A-] = 10^-3 = 0.001 M. Since pKa = 1.27, then Ka = 10^-1.27 = 0.0537. If the initial concentration of oxalic acid is c, then at equilibrium it is c - 0.001. Just substitute all we know: 0.0537 = (0.001) (0.001) / (c - 0.001) Solving, c = 0.00102 M (mole/L) The molecular weight of oxalic acid is 126 g/mol, so: (126 g/mol) (0.00102 mol/L) (0.200 L) = 0.0257 g. Just dissolve 0.0257 g of oxalic acid in 200 mL of H2O, the pH will be 3.
Answered by Glenguin - Tue Mar 10 15:18:29 2009
Q. How can I do this, knowing that the pKa of Oxalic acid is 1.27, and the volume of solution I wish to create is 200 ml or 0.2 L? Any help would be appreciated, thanks :)
Asked by TheBiochemist - Sun Mar 8 12:42:42 2009 - - 1 Answers - 0 Comments
A. Ka = [H+] [A-] / [HA] Since pH = 3, then [H+] = [A-] = 10^-3 = 0.001 M. Since pKa = 1.27, then Ka = 10^-1.27 = 0.0537. If the initial concentration of oxalic acid is c, then at equilibrium it is c - 0.001. Just substitute all we know: 0.0537 = (0.001) (0.001) / (c - 0.001) Solving, c = 0.00102 M (mole/L) The molecular weight of oxalic acid is 126 g/mol, so: (126 g/mol) (0.00102 mol/L) (0.200 L) = 0.0257 g. Just dissolve 0.0257 g of oxalic acid in 200 mL of H2O, the pH will be 3.
Answered by Glenguin - Tue Mar 10 15:18:29 2009
What's the equation for the formation of oxalic acid?
Q. I'm looking for the chemical equation. Thanks for your help.
Asked by tennisgrl9294 - Sat May 24 18:13:15 2008 - - 1 Answers - 0 Comments
Q. I'm looking for the chemical equation. Thanks for your help.
Asked by tennisgrl9294 - Sat May 24 18:13:15 2008 - - 1 Answers - 0 Comments
What is the chemical formula for oxalic acid?
Q. HOOCCOO(aq) or OOCCOO(H)2(aq) ?
Asked by Rock-Kandi - Tue Oct 27 21:02:48 2009 - - 6 Answers - 0 Comments
A. HOOCCOOH
Answered by x52raylewis - Tue Oct 27 21:09:21 2009
Q. HOOCCOO(aq) or OOCCOO(H)2(aq) ?
Asked by Rock-Kandi - Tue Oct 27 21:02:48 2009 - - 6 Answers - 0 Comments
A. HOOCCOOH
Answered by x52raylewis - Tue Oct 27 21:09:21 2009
What are the equations for the 2-step ionization of oxalic acid?
Q. What are the equations for the 2-step ionization of oxalic acid?
Asked by Marta - Tue Mar 24 19:37:35 2009 - - 1 Answers - 0 Comments
A. Step 1: C2H2O4 (aq) C2HO4- (aq) + H+ (aq) Step 2: C2HO4- (aq) C2O4-- (aq) + H+ (aq) Overall: C2H2O4 (aq) C2O4-- (aq) + 2 H+ (aq)
Answered by Glenguin - Wed Mar 25 11:40:07 2009
Q. What are the equations for the 2-step ionization of oxalic acid?
Asked by Marta - Tue Mar 24 19:37:35 2009 - - 1 Answers - 0 Comments
A. Step 1: C2H2O4 (aq) C2HO4- (aq) + H+ (aq) Step 2: C2HO4- (aq) C2O4-- (aq) + H+ (aq) Overall: C2H2O4 (aq) C2O4-- (aq) + 2 H+ (aq)
Answered by Glenguin - Wed Mar 25 11:40:07 2009
what is the Ea of reaction between oxalic acid with the potassium permanganate?
Q. i means the thoeretical activation energy. thanks!
Asked by San - Tue Jul 11 11:04:51 2006 - - 1 Answers - 0 Comments
A. The oxalic acid reacts with the potassium permanganate in a redox reaction: 2MnO4- + 6H+ + 5H2C2O4 2Mn2+ + 8H2O + 10CO2
Answered by raj - Tue Jul 11 14:35:26 2006
Q. i means the thoeretical activation energy. thanks!
Asked by San - Tue Jul 11 11:04:51 2006 - - 1 Answers - 0 Comments
A. The oxalic acid reacts with the potassium permanganate in a redox reaction: 2MnO4- + 6H+ + 5H2C2O4 2Mn2+ + 8H2O + 10CO2
Answered by raj - Tue Jul 11 14:35:26 2006
How I remove sulphate ion impurity in commercial production of Oxalic Acid?
Q. I need to bring down the sulphate impurity level to around 20 ppm from about 0.04% level.
Asked by sandysurd - Wed Jun 20 07:31:58 2007 - - 1 Answers - 0 Comments
A. Try Chromatography.
Answered by ag_iitkgp - Wed Jun 20 13:44:06 2007
Q. I need to bring down the sulphate impurity level to around 20 ppm from about 0.04% level.
Asked by sandysurd - Wed Jun 20 07:31:58 2007 - - 1 Answers - 0 Comments
A. Try Chromatography.
Answered by ag_iitkgp - Wed Jun 20 13:44:06 2007
How many grams of acid are needed to make 1L of 0.05 M oxalic acid solid ?
Q. The molecular weight of oxalic acid is 126.0
Asked by aqua girl - Tue Nov 11 02:37:09 2008 - - 1 Answers - 0 Comments
A. Moles = M x V = 0.05 M x 1 L = 0.05 mass = moles x molar mass = 0.05 mol x 126.0 g/mol= 6.3 g
Answered by Dr.A - Tue Nov 11 03:13:26 2008
Q. The molecular weight of oxalic acid is 126.0
Asked by aqua girl - Tue Nov 11 02:37:09 2008 - - 1 Answers - 0 Comments
A. Moles = M x V = 0.05 M x 1 L = 0.05 mass = moles x molar mass = 0.05 mol x 126.0 g/mol= 6.3 g
Answered by Dr.A - Tue Nov 11 03:13:26 2008
Is the oxalic acid in spinach bad for my teeth?
Q. ...It leaves them feeling very gritty.
Asked by Arch Teryx - Fri May 29 19:59:03 2009 - - 1 Answers - 0 Comments
A. 1. Any food that produces acid should not be left in your mouth for long...not even milk. So, after eating just rinse out if you cannot brush your teeth for a while. Definitely, cannot miss brushing and flossing at night. 2. With spinach in your diet, the absorption of Calcium can be less. So, if you have to take Calcium, make sure your intake of spinach is less for that period. Maybe you can switch the time for the Calcium and Spinach.
Answered by PenPress - Tue Jun 2 11:30:04 2009
Q. ...It leaves them feeling very gritty.
Asked by Arch Teryx - Fri May 29 19:59:03 2009 - - 1 Answers - 0 Comments
A. 1. Any food that produces acid should not be left in your mouth for long...not even milk. So, after eating just rinse out if you cannot brush your teeth for a while. Definitely, cannot miss brushing and flossing at night. 2. With spinach in your diet, the absorption of Calcium can be less. So, if you have to take Calcium, make sure your intake of spinach is less for that period. Maybe you can switch the time for the Calcium and Spinach.
Answered by PenPress - Tue Jun 2 11:30:04 2009
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