Tuesday
May 21, 2013

# Search: chemistry - synthesis of aspirin

Number of results: 92,122

Technology
I thought you had chemistry. Aspirin is a chemical compound. This lab is a standard in College chem labs, and HS AP Chem labs. http://en.wikipedia.org/wiki/Aspirin#Synthesis
Tuesday, January 19, 2010 at 3:18pm by bobpursley

chemistry
In the synthesis of Aspirin, would you eat your own aspirin crystals? If not, provide three (3) reasons why not?
Saturday, May 1, 2010 at 8:52am by Sue

Chemistry
Aspirin is included hut I think you can skip that and go to the next part. http://chemistryzone.blogspot.com/2010/03/synthesis-of-aspirin-how-to-prepare-oil.html
Wednesday, April 13, 2011 at 1:49pm by DrBob222

Chemistry
If 0.150 moles of salicylic acid and execs acetic anhydride are used during a synthesis of aspirin, how many grams of aspirin will be obtained if the reaction gives a 38% yield?
Saturday, April 28, 2012 at 2:20pm by Tiffany

chemistry - synthesis of aspirin
ok therefore, the mass of the aspirin is equal to the mass of the acetic acid since the ratio is 1:1. Right?
Saturday, April 7, 2012 at 8:32pm by Priscilla

chemistry
I need some help with calculating percent yield and percent purity of aspirin. Here's my data (questions follow): SYNTHESIS Mass of salicylic acid.., 2.0 g Volume of acetic anhydride.., 5 mL Mass of watch glass.., 22.10 g Mass of aspirin and watch glass.., 28.01 g Mass of ...
Saturday, March 24, 2007 at 11:33am by Jim

aspirin
during the synthesis of aspirin, why do the crystals mostly form when the test tube is placed in the ice bath and not before?
Sunday, January 24, 2010 at 5:23pm by chrissy

chemistry - synthesis of aspirin
This is an experiment for a synthesis of aspirin lab mass of salicylic acid = 2.005 g mass of acetic acid = ? moles of acetic acid = ? volume of acetic anhydride = 4 ml mass of acetic anhydride (Use 1.08 g/ml for the liquid density) = (1.08 g/ml) (4 ml) = 4.32 g moles of ...
Saturday, April 7, 2012 at 8:32pm by Priscilla

chemistry - synthesis of aspirin
ok thank you
Friday, April 6, 2012 at 4:23pm by Priscilla

chemistry
a. What is the molecular weight of aspirin (C9H8O4)? 180.1574 amu b. What is the mass of 0.00785 mol of aspirin? 1.41 g c. How many moles of aspirin are present in 100 mg of aspirin? Enter your answer in scientific notation. 5E-4 mol aspirin d. How many molecules of aspirin ...
Saturday, February 11, 2012 at 2:32pm by krystal

chemistry - synthesis of aspirin
wanted to calculate the theoretical and actual yield of aspirin. mass of salicylic acid = 2.005 g But isn't salicylic acid differ. from acetic acid? If so, how do we find the mass of acetic acid in this experiment volume of acetic anhydride = 4 ml mass of acetic anhydride...
Saturday, April 7, 2012 at 1:31pm by Priscilla

Chemistry
Aspirin is a weak acid with a Ka of 3.0x10^-5. Find the pH of a solution by dissolving .65g of aspirin in water and diluting it to 50mL. You can use RCOOH to represent aspirin. Molecular weight of aspirin is 180g/mol
Saturday, November 26, 2011 at 3:24pm by Jessica

chemistry
Aspirin is synthesized in a reaction with a theoretical yield of 0.728 moles of aspirin. What is the % yield of 1.26 g of aspirin is recovered MW of aspirin is 180.15 thank you so much!
Thursday, February 17, 2011 at 5:41pm by Dianne

Chemistry
A student was synthesizing aspirin in the lab. Using the amount of limiting reactant, she calculated the mass of aspirin that should form as 5.24g. When she weighed her aspirin product on the balance, it mass was 2.23g. What is the percent yield of the aspirin?
Wednesday, March 27, 2013 at 1:05am by Dion

chemistry lab
if you find salicylic acid or acetic anhydride in your aspirin synthesis product why are they there? Where did they come from?
Sunday, March 20, 2011 at 9:48pm by annonymous

Chemistry
Well, If 0.150 moles of salicylic acid and execs acetic anhydride are used during a synthesis of aspirin, how many grams of aspirin will be obtained if the reaction gives a 38% yield? So, let us refer to the common history of knowledge to help us answer this question. First ...
Saturday, April 28, 2012 at 2:20pm by Pundas

chemistry
Write the equation. aspirin + NaOH ==&gt; Aspirin*sodium salt + H2O 2. Calculate moles of NaOH. That will be M x L = ?? 3. The equation you have written should give you a 1:1 ratio of aspirin to NaOH. 4. Therefore, moles aspirin = moles NaOH 5. Now convert moles aspirin to...
Sunday, January 17, 2010 at 11:14pm by DrBob222

chemistry - synthesis of aspirin
Yes, what you've written is right. Why are you worrying about acetic acid? That's a product but you want theoretical yield of aspirin so how much acetic acid is produced is of no interest. If you wanted theoretical yield of acetic acid we would be interested in that ...
Saturday, April 7, 2012 at 1:31pm by DrBob222

chemistry lab
Probably they came from the stock room or wherever chemicals are stored at your facility. Both are starting materials for the synthesis of aspirin.
Sunday, March 20, 2011 at 9:48pm by DrBob222

Chemistry
A student carried out the synthesis of aspirin, starting with 3.22 g of salicylic acid. After carrying out the reaction, recrystallizing and then drying the product, the student obtained 3.65 g of aspirin. Calculate the percent yield. I'm pretty sure it's (3.65 g / 3....
Monday, March 30, 2009 at 10:19pm by John

chemistry characterization & analysis of aspirin
Aspirin is C9H8O4 and it has one acid H on it so I will rewrite it as HC9H7O4. HC9H7O4 + NaOH ==&gt; NaC9H7O4 + H2O If you know the molarity of the NaOH and measure mL required for titration, then mol aspirin = M NaOH x L NaOH = mols NaOH = mols aspirin. You can see the ...
Tuesday, November 13, 2012 at 12:10am by DrBob222

chemistry
Here is an excellent discussion of the synthesis of aspirin. http://wwwchem.csustan.edu/consumer/aspirincons/aspirincons.htm hint: Look at the decomposition of unreacted acetic anhydride and recrystallization of aspirin.
Sunday, March 20, 2011 at 9:54pm by DrBob222

chemistry - synthesis of aspirin
No. Mass of acetic acid = mols acetic acid x molar mass acetic acid and that is the theoretical yield of acetic acid in grams. I don't know the exact instructions you have but if I were asked to calculate grams acetic acid produced I would do as above then multiply by the ...
Saturday, April 7, 2012 at 8:32pm by DrBob222

chemistry - synthesis of aspirin
1 mol acetic anhydride + 1 mol salicylic acid = 1 mol aspirin I don't know the formulas (I could look them up but you probably have them) but the above tells you what you want to know. It's a 1:1 ratio throughout. You will need to calculate the mols salicylic acid and ...
Friday, April 6, 2012 at 4:23pm by DrBob222

chemistry - synthesis of aspirin
wait, I just have one quick question. I realized the equation for this experiment would be C7H6O3 + C4H6O3 ----&gt; C9H8O4 + C2H4O2 BUT... acetic acid's formula is C2H402 in molecular formula. Is the above equation right? Also, I realized after mixing salicylic acid ...
Friday, April 6, 2012 at 4:23pm by Priscilla

Chemistry
If we call aspirin, HA, then the acid dissociates in water as HA ==&gt; H^+ + A^- Ka = (H^+)(A^-)/(HA) (H^+) = x (A^-) = x (HA) = moles aspirin/L soln. moles aspirin = 2*500/molar mass aspirin. L soln = 0.325 L Solve for x and convert to pH. Post your work if you get stuck.
Wednesday, December 8, 2010 at 11:00am by DrBob222

chemistry - synthesis of aspirin
I checked your values for mols aspirin and it looks good except I would carry it out one more place. You have 3 significant figures in all of the other numbers (if the 4 mL is 4.00 mL); therefore, you can have 3 in the 0.012 number. Same for mols acetic anhydride; again I'...
Saturday, April 7, 2012 at 8:32pm by DrBob222

Jim
I need some help with calculating percent yield and percent purity of aspirin. Here's my data (questions follow): SYNTHESIS Mass of salicylic acid.., 2.0 g Volume of acetic anhydride.., 5 mL Mass of watch glass.., 22.10 g Mass of aspirin and watch glass.., 28.01 g Mass of ...
Saturday, March 24, 2007 at 12:37am by Chemistry

organic chemistry
1. why is phosphoric acid needed in the synthesis of aspirin? 2.what would happen if the phosphoric acid is left out?
Wednesday, March 17, 2010 at 6:16pm by 10ch

chemistry
can anyone help me with the following question? 1. why is phosphoric acid needed in the synthesis of aspirin? 2.what would happen if the phosphoric acid is left out?
Wednesday, March 17, 2010 at 6:16pm by HH

Chemistry
The rxn is 1:1 meaning that 1 mol aspirin is produced from 1 mol salicylic acid. Therefore, 0.150 mol S.A will produce 0.150 mol aspirin. That is the theoretical yield. That x 0.38 will give you the actual yield in mols and mols x molar mass aspirin = grams aspirin actually ...
Saturday, April 28, 2012 at 2:20pm by DrBob222

(5.0ml)x(2.0g/1.08g/ml)x(1 mole S/138g S) x (1 mole Aspirin/1 mole S)x (180g Aspirin/ 1 mole Aspirin) = 12.077 g Aspirin
Sunday, April 20, 2008 at 5:53pm by Sara

chemistry
The distribution coefficient between ether & water for aspirin at room temperature is 3.5. What weight of aspirin would be extracted by a single extraction with 150 ml water from a solution of 10 gms of aspirin in 100 ml ether? Calculate the weight of aspirin which would ...
Monday, June 18, 2012 at 11:25am by nimfa

chemistry
aspirin tablets contain about 5 grains of aspirin. About 10 grams of aspirin constitute a fatal dose. How many tablets would this be? (There are approximately 15 grains in a gram)
Saturday, October 22, 2011 at 5:27pm by Jay

chemistry
How many grams of aspirin is equlvalent to 150 mg of aspirin?
Wednesday, September 15, 2010 at 5:44pm by janay

chemistry
How many 400-mg aspirin tablets can be made from 40.0-kg of aspirin?
Wednesday, January 18, 2012 at 1:51pm by Cynthia

chemistry
A 0.010 M solution of aspirin, a weak monoprotic acid, has a pH of 3.3. What is the Ka of aspirin?
Thursday, September 9, 2010 at 7:36am by Martha

chemistry
FeCl3 will not react with aspirin. It will, however, react with salicylic acid, which is used to synthesize aspirin. Thus by adding an aqueous FeCl3 solution to a sample of aspirin is a good way to see if there is any unreacted salicylic acid. A purple colour is an indication ...
Friday, December 18, 2009 at 4:00am by Dr Russ

chemistry
How many moles of aspirin are present in 100 mg of aspirin? Enter your answer in scientific notation. 5.5E-4
Monday, February 13, 2012 at 3:11pm by krystal

chemistry - synthesis of aspirin
I wanted to calculate the theoretical and actual yield of aspirin. mass of salicylic acid = 2.005 g But isn't salicylic acid differ. from acetic acid? If so, how do we find the mass of acetic acid in this experiment volume of acetic anhydride = 4 ml mass of acetic ...
Friday, April 6, 2012 at 4:23pm by Priscilla

Chem Lab
Aspirin synthesis and Analysis: Calculate theoretical yield of ASA? Used 3.5mL of acetic anhydride and 1.5g of salicylic acid.
Friday, November 2, 2012 at 12:52am by Cris

chem
Are aspirin, starch and dextrose covalent or ionic? Do aspirin and or epsom salt conduct electricity? Any help with these questions would be greatly appreciated. Thank you! I have been told by more than one person that aspirin often is sold as the sodium salt; however, aspirin...
Thursday, February 1, 2007 at 6:14pm by Fidelia

chemistry - synthesis of aspirin
Okay i understand from what you said. But in my lab report, they stated the mass of acetic acid and from that I would have to calculate the number of moles of acetic acid. But since you state acetic acid is just a product should i leave these two questions blank then
Saturday, April 7, 2012 at 1:31pm by Priscilla

chemistry
assume all of the ionized aspirin remains in the buffer solution and all of the un-ionized aspirin goes into to the ethyl acetate, what is the molarity of the aspirin in the ethyl acetate at pH 2 and pH 8? what equation would ou use for this?
Wednesday, April 3, 2013 at 8:31pm by kelly

chemistry characterization & analysis of aspirin
write a balanced equation that describes an acid base reaction that would allow you to determine the moles of aspirin present in a sample
Tuesday, November 13, 2012 at 12:10am by molly

chemistry
You may be looking for the word "synthesis." 2Mg + O2 ==&gt; 2MgO is a synthesis reaction.
Tuesday, September 14, 2010 at 2:30am by DrBob222

Social Studies Aspirin Project
When/ where/ why was Aspirin invented? Who thouht of it? Does anyone have good project ideas? I think I might make the poster in a pill shape and put on an empty box of Aspirin but I'm not sure.
Thursday, January 29, 2009 at 3:41pm by Twilight lover

Chemistry
Use the coefficients in the balanced equation. mols SA x (2 mols aspirin/2 mols SA) = mols SA x 2/2 = ? mols aspirin. mols AA x (2 mols aspirin/1 mol AA) = mols AA x 2/1 = ? mols aspirin.
Sunday, September 23, 2012 at 11:57pm by DrBob222

Chemistry
Yes for ether. You don't know grams aspirin so you can't calculate moles aspirin. Subtract normal vp ether - vp ether desired, plug into pether = Xether*Po ether and solve for Xether. Then find Xaspirin (it's 1.000 - Xether) and from that grams aspirin. It's ...
Sunday, February 19, 2012 at 5:34pm by DrBob222

chem
he literature value for the melting point of aspirin is 135°C. Suppose that a sample of aspirin prepared in Experiment 41 melts over the temperature range 125–128°C. What does this result suggest about the purity of this sample of aspirin?
Tuesday, May 10, 2011 at 9:57am by maribel

Chemistry
If you check week 12: Amino Acids and Protein Synthesis, S32E5: SYNTHESIS OF PEPTIDES, you can work your way through this problem...
Friday, January 11, 2013 at 9:03am by Anonymous

science
Can some one help me I don’t know what to take out from the aspirin molecule, for the following structures? I have to generate a copy of the molecular structure of aspirin and then for each of the molecular features listed in (i) – (iii) have to produce a related ...
Friday, June 29, 2007 at 6:41pm by katie

Chemistry
The LD (subscript 50) for a drug dose that would be fatal for 50% of the population. The LD (subscript 50)for aspirin in rats is 1.75 grams/kilogram of body weight. Calculate how many aspirin tablets a human weighing 155 pounds would have to take to reach this dosage. (1 ...
Sunday, January 8, 2012 at 2:49am by Sharon

Chemistry
A student performed the synthesis of aspirin using a water bath at 90C instead of 50C. The final product was tested for the presence of phenols with ferric chloride. This test was negative (no color observed); however, the melting point of the dry product was 122-125 C. ...
Saturday, March 20, 2010 at 8:24pm by Sunny

chemistry
A student performed the synthesis of aspirin using a water bath at 90C instead of 50C. The final product was tested for the presence of phenols with ferric chloride. This test was negative (no color observed); however, the melting point of the dry product was 122-125 C. ...
Wednesday, March 17, 2010 at 7:06pm by 10ch

chemistry
x = wt aspirin in ether 10-x = st aspirin in H2O layer. 3.5 = (x/100)/(10-x/150 Solve for x and 10-x
Monday, June 18, 2012 at 11:25am by DrBob222

Chemistry
write and balance the chemical reaction. change 75g aspirin to moles of aspirin. Now multiply that by 1/.682. Now, use the mole ratio to determine each reactant from the balanced formula.
Wednesday, October 8, 2008 at 8:40pm by bobpursley

chemistry
2 C7H6O3 + 1 C4H6O3 -&gt; 2 C9H8O4 + H2O 45.0 g / 0.85 = 52.9 g theoretical yield. 52.9 g C9H8O4 x (1 mole / 180.2g) = 0.294 moles aspirin 0.294 moles aspirin x (2 moles C7H6O3 / 2 moles aspirin) x (138.1 g C7H6O3 / mole C7H6O3) = 40.6 g salicylic acid. 0.294 moles aspirin...
Wednesday, October 18, 2006 at 7:25pm by Anonymous

chem
Convert 14 g salicylic acid to moles. Moles = grams/molar mass. Convert 8.5 g acetic anhydride to moles the same way. Since this is a 1:1 ratio, the moles of salicylic acid will be the same as the moles of aspirin produced. Next, since this is a 1:1 ratio, the moles of acetic ...
Tuesday, September 1, 2009 at 3:51pm by DrBob222

chemistry - synthesis of aspirin
wait, i misunderstand. You stated that if there's no H2O present then salicylic acid is the limiting reagent. Therefore salicylic acid number of moles is the same as the number of moles of acetic acid???? If this is so, then the mass of acetic acid would also be 2.005 g, ...
Saturday, April 7, 2012 at 8:32pm by Priscilla

chem
Aspirin, C9H8O4, is produced from salicylic acid, C7H6O3, and acetic anhydride, C4H6O3: C7H6O3 + C4H6O3 --&gt; C9H8O4 + HC2H3O2 a. How much salicylic acid is required to produce 1.5 x 10^2 kg of aspirin, assuming that all of the salicylic acid is converted to aspirin? b. ...
Friday, August 17, 2012 at 1:39pm by greeny

chemistry
Can you please explain the buffer system used in buffered aspirin? For example, what is the chemical formula of the buffer that is used? How does it react with the aspirin?
Tuesday, June 14, 2011 at 7:17pm by Jessica

chemistry - synthesis of aspirin
Now you're confusing me. I have made some assumptions in answering your questions. Some of those assumptions may not be right if the questions change; please type everything in and I can have ALL of the information at one time instead of getting it in bits and pieces. From...
Saturday, April 7, 2012 at 1:31pm by DrBob222

Chemistry
Regarding your first post, I believe I used aspirin as the weak acid. In a previous problem which was related to these problems, it stated "aspirin is a weak acid with a Ka of 3.0x10^-5"
Saturday, November 26, 2011 at 8:14pm by Jessica

chemistry
describe basic steps to take re-crystalizing synthesized aspirin. using two solvents to perform this task (ethanol and water)which solvent should be used to dissolve the aspirin and which one should force it out of the solution
Tuesday, November 13, 2012 at 4:51pm by morgan

chemistry
The evaporation procedure must be completed in 10-15 minutes right after isolating aspirin in the filtration step with alumina or the aspirin decomposes which will create more surface area on the molecule resulting a lower melting point and wider temperature range.
Saturday, October 17, 2009 at 9:26pm by nadine

chemistry
Acetylsalicyclic Acid, HC9H704, is the active component is aspirin. Two extra strength aspirin tablets, each containing 500 mg of acetylsalicylic acid, are dissolved in 325 ml of water. What is the pH of teh solution? (Assume Ka=3.3x10^-4)
Sunday, December 5, 2010 at 8:53pm by Symone

Chemistry-help
How does a "chemical for synthesis" compare with the same chemical(ACS grade)when used in analytical testing? Posted by candy on Tuesday, January 11, 2011 at 2:10pm. Chemicals are supplied in different grades,e.g. ACS,AR...etc.What do we mean when we say that the ...
Wednesday, January 12, 2011 at 3:23pm by candy

chemistry re crystalizing
describe basic steps to take re-crystalizing synthesized aspirin. using two solvents to perform this task (ethanol and water)which solvent should be used to dissolve the aspirin and which one should force it out of the solution
Tuesday, November 13, 2012 at 1:43am by justin

Chemistry- helpp!
The equation for synthesis of the poisonous gas COCl2 is CO(g) + Cl2(g)COCl2 If 43.2 kJ of energy is evolved when 39.5 g of COCl2 is synthesized, what is the molar enthalpy for this synthesis? THANK YOU!
Tuesday, November 2, 2010 at 5:24pm by Melissa

chemistry
assuming that 1g of aspirin dissolves in 450ml of water at 10Â°C,how much aspirin would be lost in the 5ml of water added to the reaction mixture if the mixture were at 10Â°C during filtration?
Monday, August 16, 2010 at 3:26pm by kabelo

Chemistry
Aspirin is prepared by heating salicylic acid, C7H6O3, with acetic anhydride, C4H603. The other product produced is acetic acid, C2H402. C7H6O3+C4H6)3-&gt;C9H8O4+C2H4O2 What is the theoretical yield in grams of aspirin, C9H8O4, when 2.00 grams of salicylic acid is heated ...
Tuesday, November 6, 2012 at 8:00pm by Lauren

chemistry
Use the density to calculate the mas of the 175 mL ethanol. Add mass ethanol to mass aspirin. mass % = (mass aspirin/total mass)*100 = ?
Tuesday, November 29, 2011 at 3:12am by DrBob222

Chemistry
mols SA = 19/molar mass SA. mols AA = 19/molar mass AA. Convert mols of SA to mols of aspirin (use the coefficients in the equation). Convert mols AA to mols of aspirin(use the coefficients here too). The reagent giving the smallest number for mols aspirin is the limiting ...
Sunday, September 23, 2012 at 11:57pm by DrBob222

chemistry
C7H6O3 (s) + C4H6O3 (l) -&gt; C9H8O4 (s) + C2H4O2 (l) molar masses: salicylic acid, C7H6O3 = 138.12 g/mol acetic anhydride, C4H6O3 = 102.09 g/mol Asprin, C9H8O4 = 180.157 g/mol For this problem calculate the moles of aspirin obtained from 45.0 g. This represents an 85.0% ...
Wednesday, October 18, 2006 at 7:25pm by Anonymous

math
A veterinarian has instructed Harrison to give his 75lb dog one 325 mg aspirin tablet for arthritis. the amount of aspirin A remaining in the dog's body after t minutes can be expressed by A=325(1/2)^(t/15). write and solve a logarithmic inequality to find the time it ...
Wednesday, February 20, 2008 at 7:22pm by yaz

Chemistry
In life terms it is metabolism but you want the term decomposition for chemical reaction. There are synthesis, decomposition, single replacement, and double replacement. Decomposition is the reverse of synthesis.
Sunday, October 2, 2011 at 11:48pm by DrBob222

chemistry
Assuming that 1 gram of aspirin dissolves in 450 ml of water at 10°C, how much aspirin would be lost in 40 ml of water added to the reaction mixture if the mixture were at 10 °C during filtration?
Tuesday, April 20, 2010 at 8:59pm by bobby

Chemistry
The melting point of aspirin : 128-137Celsius degree. The melting point of the crude aspirin was measured to be 128 Celsius degree. What does it indicate about the purity of the product?
Sunday, December 5, 2010 at 10:27pm by Cynthia

Biochem
The theory of ATP synthesis by the ATP synthesis apparatus is called the _______ theory. I have no idea. Can some please help? Go to www.google.com and type in "ATP synthesis" without the parentheses. I think you will find your answer about four or five references ...
Thursday, July 20, 2006 at 5:05pm by shamaev

Chemistry
Aspirin can be prepared by the reaction of salicylic acid with an excess of acetic anhydride, using phosphoric acid as a catalyst. Once the aspirin is formed, it is precipitated from the reaction mixture by adding water and filtering. The solid aspirin obtained in this way is ...
Thursday, April 2, 2009 at 4:29pm by Paul

Chemistry
There are advantages (and disadvantages) for aspirin here http://en.wikipedia.org/wiki/Aspirin and acetaminophen (paracetemol) here http://en.wikipedia.org/wiki/Acetaminophen Certainly one of the main advantages of paracetemol over aspirin is the reduction in gastrointestinal ...
Monday, October 11, 2010 at 5:51am by Dr Russ

AP CHEMISTRY
What is the of a solution obtained by dissolving two extra-strength aspirin tablets, containing 594 of acetylsalicylic acid each, in 202 of water? The active ingredient in aspirin is acetylsalicylic acid , a monoprotic acid with Ka=3.3*10^-4 at 25 C. Can you provide the method...
Wednesday, January 2, 2013 at 9:51pm by Amber

chem
What didn't work when you typed it before? I worked this problem for someone, perhaps you and perhaps another student. But let me point out that the problem does not state what it is tht goes in the blank. I know concn but concn of what? Is it concn of the aspirin tablet; ...
Sunday, April 20, 2008 at 6:01pm by DrBob222

Social Studies Aspirin Project
By the way, the poster is about HOW Aspirin was invented. We're learning about the Industrial Revolution.
Thursday, January 29, 2009 at 3:41pm by Twilight lover

Chemistry
A student who was isolating aspirin stopped the experiment after filtration step alumina. One week later, the methanol was evaporated and the experiment was completed. The melting point of the aspirin was found to be 110-115 degrees C. Explain why the melting point was low and...
Friday, October 10, 2008 at 3:46pm by Nina

chemistry
Mass of Aspirin tablet: 0.357 g 10 mL of 1 M NaOH was added to the aspirin tablet in a 125 mL Erlenmeyer flask and heated to a boil. The solution was transferred to a 100 mL volumetric flask and the flask was filled to the mark with DI water. 1 mL of the solution was pipetted ...
Sunday, January 31, 2010 at 4:02am by t

chemistry
Look for mol Mass in the right panel. http://en.wikipedia.org/wiki/Aspirin
Saturday, June 12, 2010 at 12:02pm by DrBob222

Chemistry
Until that time, everyone thought that the synthesis (creation) of organic compounds required a "vital force" or a "living force." Wohler's synthesis showed that was not the case. He synthesized an organic compound in the lab without using a living cell.
Monday, January 24, 2011 at 9:15pm by DrBob222

Chemistry
A + B ==&gt; AB synthesis AB + CD ==&gt; AC + BD double replacement AB ==&gt; A + B decomposition (the reverse of synthesis) etc. There must be something fundamental going on here. Perhaps I can help if you can be specific about your understanding of this concept.
Tuesday, April 5, 2011 at 12:14am by DrBob222

HONORS CHEMISTRY
A synthesis of nitrogen dioxide from nitrogen and oxygen. There are 5.000 mol of N2 and 8.000 mol of O2 mixed in a 5.000-L flask. What is the equilibrium constant for the synthesis?
Wednesday, March 17, 2010 at 2:51am by helpless

Stats
In a study that was highly published doctors discovered that aspirin helps prevent heart attacks. The research project which was scheduled to last 5 years employed 22,000 american physicians (all male). Half took an aspirin tablet 3 times a week while the other half took a ...
Tuesday, February 27, 2007 at 9:06am by kristen

science
can any one tell me how the distance between the oxygen atom joined to the ring and the -OH group of the carboxylic acid in aspirin ... can relieve pain? For example what would be the effect of increasing the distance ? Here is a LONG discussion of aspirin, much of it ...
Thursday, July 26, 2007 at 5:00pm by kat

org. chem.
A student who was isolating aspirin stopped the experiment after the filtration step with alumina. One week later, the methanol was evaporated and the experiment was completed. The melting point of the aspirin was found to be 110-115 degress Celsius. Explain why the melting ...
Tuesday, October 6, 2009 at 5:23am by CM

AP CHEM
Aspirin has the structural formula below. Which functional groups does this molecule contain? I. Acid II. Alcohol III. Ester IV. Ether I have no way of posting the structure, but it is on google images! If you type in aspirin structural formula, it's the first one. Answer ...
Friday, April 5, 2013 at 2:58pm by Anonymous

Chemistry
The vapor pressure of chloroform is 173.11 mm Hg at 25 degrees celsius. A nonvolatile, nonelectrolyte that dissolves in chloroform is aspirin. Calculate the vapor pressure of the solution at 25 degrees celsius when 6.243g of aspirin (180.1g/mol) are dissolved in 244.5g of ...
Sunday, February 19, 2012 at 3:30pm by Hannah

Chem
(A^-)/(HA) = 0.01 tells us that the ionized portion of aspirin is MUCH less than the unionized portion; i.e. that little ionization has taken place and that most of the aspirin is in its original unionized form. That is that the (A^- or the ionized part) part is very low and ...
Sunday, July 26, 2009 at 9:51pm by DrBob222

The vapor pressure of chloroform is 173.11 mm Hg at 25 degrees celsius. A nonvolatile, nonelectrolyte that dissolves in chloroform is aspirin. Calculate the vapor pressure of the solution at 25 degrees celsius when 6.243g of aspirin (180.1g/mol) are dissolved in 244.5g of ...
Sunday, February 19, 2012 at 4:16pm by Hannah

organic chemistry
The isolation process of aspirin was stopped after the filtration step with alumina and one week later the methanol was evaporated and the experiment was completed. The melting point of the aspirin was found to be 110-115 Celsius. explain why the meltingpoint was low and why ...
Monday, October 4, 2010 at 1:32am by Tammy

chemistry
A student decided to extract aspirin from a tablet. After the alumina filtration step, he stopped the experiment for a week. then he evaporated the methanol and completed the procedure. the melting point of his recovered material was 120-145 degrees Celsius. what does this ...
Saturday, October 17, 2009 at 9:26pm by jessica

Pages: 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | Next>>