Number of results: 34,198
chemistry
given the density of acetic anhydride to be 1.05 g/mL, what was the mass of the acetic anhydride added to the reaction? How many moles of acetic acid were added?
Tuesday, March 29, 2011 at 8:44pm by kendalyn
chemistry
For the theoretical yield, I used the mass of acetic anhydride. Was I supposed to use the mass of salicylic acid (which was 2.00 g) instead? acetic anhydride + salicylic acid ---> acetic acid +acetylsalicylic acid
Wednesday, April 4, 2012 at 3:11pm by casey
chemistry
You must first determine which is the limiting reagent; i.e., salicylic acid or acetic anhydride. And you need the density of acetic anhydride to do that. mols salicylic acid = grams/molar mass = ? mols acetic anhydride = grams/molar mass. grams you get by grams = volume x ...
Friday, June 1, 2012 at 7:43am by DrBob222
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
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
Chemestry
Aspirin (C9H8O4) is synthesized by reacting salicylic acid (C7H6O3) with acetic anhydride (C4H6O3). The balanced equation is given below. C7H6O3 + C4H6O3 C9H8O4 + HC2H3O2 (a) What mass of acetic anhydride is needed to completely consume 4.20 102 g salicylic acid? g (b) What is...
Thursday, February 2, 2012 at 10:02pm by Jocelyn
AP Chemistry
Aspirin (C9H8O4) is synthesized by reacting salicylic acid (C7H6O3) with acetic anhydride (C4H6O3). The balanced equation is given below. C7H6O3 + C4H6O3 C9H8O4 + HC2H3O2 (a) What mass of acetic anhydride is needed to completely consume 4.40 102 g salicylic acid? What is the ...
Monday, August 30, 2010 at 5:36pm by BB
Chemistry
Two people were given 1.75 g salicylic acid and 2.00 mL of acetic anhydride. If the density of acetic anhydride is 1.0820 g/mL, how many grams of aspirin could they have prepared. Is the answer 4.7 g
Friday, November 14, 2008 at 11:42pm by George
Chemistry
Aspirin, C9H8O4, is produced through the following reaction of salicylic acid, C7H6O3, and acetic anhydride, C4H6O3: C7H6O3(s) + C4H6O3(l) → C9H8O4(s) + HC2H3O2(l). a.) What mass of aspirin (in kg) could be produced from 75.0 mol of salicylic acid? b.) What mass of ...
Thursday, February 19, 2009 at 8:52pm by Emat
chemistry
C7H6O3 (s) + C4H6O3 (l) -> 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
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
O Chemistry
In the reaction p-aminophenol + acetic anhydride --> acetaminophen , 4.5 ml of water is added into the flask with the p-aminophenol and acetic anhydride at the beginning of the experiment. What is the purpose of this water?
Sunday, April 4, 2010 at 12:42am by Tammy
chemistry
If you used 0.155 mL of acetic anhydride, and 0.169 g of p-aminophenol what was the limiting reagent? Choice is either: 1. acetic anhydride or 2. p-aminophenol ________mol? How many moles of the non-limiting reageant remained after the reaction was complete?
Wednesday, October 19, 2011 at 1:47am by ej
chemistry
Have you written the equation? It is a 1:1 reaction (1 mole SA and 1 mole acetic anhydride produces 1 mole aspirin). Convert 1.5 g SA to moles. mols = grams/molar mass. Convert 4 mL acetic anhydride to grams (using density), then to moles. Convert moles SA to moles product (...
Monday, April 19, 2010 at 5:23pm 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
Chemistry
You don't have enough information in the post to answer the question. I assume this is an aspirin problem and you're starting with acetic anhydride and salicylic acid and you want to know how much acetic acid is produced then calculate the volume from the mass. ...
Monday, February 6, 2012 at 11:49pm by DrBob222
Chemisty
How to calculate teh theoretical yield of aspirin to be obtained when 2.0 g of salicylic acid and 5.0 mL of acetic anhydride (density = 1.08 g/mL) are mixed together? ( Molar masses: acetic anhydride = 102.1 g/mol; salicylic acid = 138.2 g/mol)
Wednesday, January 6, 2010 at 11:54pm by Kerrie
chemistry - synthesis of aspirin
wait, I just have one quick question. I realized the equation for this experiment would be C7H6O3 + C4H6O3 ----> 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
Ask your teacher or instructor for a chemistry supplies catalog. The catalog will give you the prices. If you are using salicylic acid and acetic anhydride as the reactants, it would be far more convenient to use an excess of acetic anhydride, a liquid, since the unreacted ...
Friday, November 21, 2008 at 9:10pm by GK
chemistry
Write and balance the equation; however I think the ratio is 1:1 for reactants and products. When amounts are given for both reactants you know it is a limiting reagent problem. mols salicylic acid = grams/molar mass Look up the density of acetic anhydride and determine grams ...
Sunday, January 27, 2013 at 8:14pm by DrBob222
Chemistry
Aspirin is prepared by heating salicylic acid, C7H6O3, with acetic anhydride, C4H603. The other product produced is acetic acid, C2H402. C7H6O3+C4H6)3->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
Asprin, C9H8O4, is prepared by reacting salicylic acid, C7H6O3, with acetic anhydride, C4H6O3, in the reaction C7H6O3(s) + C4H6O3(l) -> C9H8O4(s) + C2H4O2(l) A student is told to prepare 45.0 g of aspirin. She is also told to use a 55.0% excess of the acetic anhydride ...
Wednesday, October 18, 2006 at 7:25pm by Chris
chemistry
Is it possible to make acetic anhydride from acetic acid/glacial?
Saturday, September 24, 2011 at 10:30am by irfan
O Chemistry
Do you suppose it converts the acetic anhydride to acetic acid?
Sunday, April 4, 2010 at 12:42am 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
Aspirin (C9H8O4) is synthesized by reacting salicylic acid (C7H6O3) with acetic anhydride (C4H6O3). The balanced equation is given below. C7H6O3 + C4H6O3 C9H8O4 + HC2H3O2 What mass of acetic anhydride is needed to completely consume 3.60 x 10^2 g salicylic acid? i worked out ...
Friday, January 23, 2009 at 7:52pm by lyne
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
P2O5 is the anhydride of H3PO4. As2O5 is the anhydride of H3AsO4. N2O5 is the anhydride of HNO3. SnO2 is the anhydride of Sn(OH)4 BaO is the anhydride of Ba(OH)2 You know which are strong acids or bases; therefore, those go at the top (for weakest acid) to bottom (for ...
Sunday, November 25, 2012 at 5:17pm by DrBob222
CHEM HELP
I asked this already but for some reason the answer I got isnt being accepted online Question: In the laboratory, 3.50 grams of salicylic acid were reacted with 7.20 ml of acetic anhydride (density equal to 1.08 g/ml). Determine the limiting reagent. I did: salicylic acid + ...
Tuesday, November 27, 2012 at 1:34am by Yaw
chemistry
mols acetic anhydride = grams/molar mass g acetylsalicylic acid = mols x molar mass.
Wednesday, April 4, 2012 at 3:08pm by DrBob222
chem
Aspirin (C9H8O4) is produced from salicylic acid (C7H6O3), and acetic anhydride (C4H6O3): C7H6O3 + C4H6O3 ¨ C9H8O4 + HC2H3O2 . (c) What is the theoretical yield of aspirin if 189 kg of salicylic acid is allowed to react with 128 kg of acetic anhydride? (d) If the ...
Sunday, October 7, 2012 at 8:12pm by rebekah
chemistry (Pls Bob check for me)
Aspirin c9h8oh molar mass = 180.1g/mol can be prepared by the reaction of salicylic acid c7h603 molar mass = 13801 g/mol with acetic anhydride c6h603, according to the following equation. A chemist starts with 2 gram of salicylic acid reacts it with excess acetic anhydrate, ...
Sunday, April 28, 2013 at 2:28pm by Fai
chemistry
Molar mass of salicylic acid: C6H4(OH)CO2H = 138.12074 g/mol acetic anhydride: Molecular formula, C4H6O3. Molar mass, 102.09 g/mol You should be able to take it from there.
Friday, February 24, 2012 at 8:46am by Steve
Chem(check my work, mass percent acetic acid)
I do believe this is the right annswer (.11g Acetic Acid present). When you you use the above equation for the mass percent of acetic acid (g CH3COOH/g sample) you end up with 4.3% Acetic Acid. That is a normal concentration of acetic acid [I looked at other sites for ...
Monday, June 12, 2006 at 1:20pm by BRAD
chemistry
how'd you get 1.55g acetic anhydride?
Wednesday, October 18, 2006 at 7:25pm by Anonymous
Chemistry
ASpirin, c9h8o4, is prepared by reating salicylic acid, c7h6o3, with acetic anhydride, c4h6o3, in the reaction. c7h6o3 + c4h6o3---> c9h8o4 + c2h4o2 A student is told to prepare 45.0 g of aspirin. she is also told to use a 55.0 % excess of acetic anhydride and to expect ...
Monday, September 22, 2008 at 11:06pm by Komal
Chemistry
SA = salicylic acid AH = acetic anhydride SA + AH ==> acetic acid + ASA(aspirin) mols SA = 2.489/molar mass SA. Convert to mols ASA. mols ASA = mols SA g ASA = mols ASA x molar mass ASA (this is the theoretical yield).
Tuesday, February 12, 2013 at 2:35pm by DrBob222
Chemisty
Most of these stoichiometry problems are worked the same way. This problem is a limiting reagent problem and stoichiometry rolled into one. 1. Write and balance the equation. 2. Convert g salicylic acid to moles. Moles = grams/molar mass. Convert 5.0 mL acetic anhydride (using...
Wednesday, January 6, 2010 at 11:54pm 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
Chem Lab
This is a limiting reagent problem and you don't have enough information to work the problem. You have 3.5 mL acetic anhydride and you need to convert that to mols. You need the density of the acetic anhydride to convert 3.5 mL to grams. Here is a site that will show you ...
Friday, November 2, 2012 at 12:52am by DrBob222
Chemistry
Asprin, c9h804, is produced through the following reaction of salicyclic acid, c7h6o3, and acetic anhydride, c4h6o3. chemical equation: c7h6o3 + c4h6o3 yields c9h8o4 + hc2h3o2 (all numbers in this equation are subscripts) At 20 degrees Celsius. how many liters of acetic acid, ...
Sunday, January 21, 2007 at 2:18am by Steph
chemistry
How many grams of acetic anhydride are needed to react with 3.25 of salicylic acid?
Thursday, August 26, 2010 at 6:36pm by Anonymous
Law
looking to ascertain what the liquid volume of 5 gallons of acetic anhydride is in pounds.
Monday, April 25, 2011 at 6:24am by kevin
chem
Aspirin, C9H8O4, is produced from salicylic acid, C7H6O3, and acetic anhydride, C4H6O3: C7H6O3 + C4H6O3 --> 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
Asprin C9H8O4 is made by the reaction of salicylic acid C7H6O3 and acetic anhydride C4H6O3. The other product in the reaction is acetic acid HC2H3O2. How many of each reactant should be used to produce 75.0g of asprin. Assume that the reaction gives a 68.2% yield.
Wednesday, October 8, 2008 at 8:40pm by Mookie
chemistry
density = 1.0187 g/mL. mass 1000 mL = 1.0187 x 1000 mL = ?? How much of that is acetic acid? 15%; therefore, ?? x 0.15 = mass acetic acid = xx. How many mols is that? xx g acetic acid/molar mass acetic acid = yy Molarity = yymols/L = yy M. molality = mols solute/kg solvent ...
Monday, February 11, 2008 at 9:01pm by DrBob222
Chemistry
a. 75 mol of salicylic acid will product 75.0 mol aspirin since 1 mol of salicylic acid produces 1 mol aspirin. Then grams = mols x molar mass. b. You know 75.0 mol salicylic acid will require 75.0 mol acetic anhydride. g = mols x molar mass. c. 75.0 moles salicylic acid will ...
Thursday, February 19, 2009 at 8:52pm by DrBob222
Chemistry
What is the theoretical yield of aspirin if you have 2g of salicylic acid and 5 ml acetic anhydride?
Tuesday, April 19, 2011 at 12:18am by N/A
Chemistry
Writ the equation for salicylic acid + acetic anhydride to produce ASA. This is a limiting reagent problem. 2a. Convert 2.0 g salicylic acid to mols. 2b. convert 5.0 mL to grams by density, then to mols. 3. Convert to mols ASA (aspirin) a. Convert mols salicylic acid to mols ...
Sunday, April 20, 2008 at 5:53pm 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
CO2 + H2O ==> H2CO3 (carbonic acid). Know what CO2 dissolved in water (to make carbonated drinks) contains? H2CO3. So CO2 is the anhydride of H2CO3. SO2 is the anhydride of H2SO3. SO3 is the anhydride of H2SO4. N2O5 is the anhydride of HNO3. (The anhydride of HNO3 is ...
Sunday, May 31, 2009 at 7:21pm by DrBob222
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
2 C7H6O3 + 1 C4H6O3 -> 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
Chemistry
what is the theoretical yield in grams of aspirin if 2.04g of salicycli acid reacts with an excess of acetic anhydride ?
Monday, September 26, 2011 at 7:31pm by Kay
Chemistry
If 2 g of salicylic acid is heated with 4 g of acetic anhydride, what is the theoretical yield ? C7H6O3 + C4H6O3 --> C9H8O4 + C2H4O3
Saturday, April 17, 2010 at 10:45pm by Fiona
ChEMISTRY (Help please)
Calculate the mass percent of acetic acid in acetic acid solution. Average molarity= .8806753M Average density= 3.27463 Molar mass of acetic acid= 60.042g
Tuesday, April 13, 2010 at 8:02pm by Michelle
chemistry
The molar mass of acetic acid is 24+4+32=60 Then, There is 0.201 mol acetic acid per litre or 0.201*60=12.06g of acetic acid The density is 1g/ml to change to g/l it becomes 1000g/l then the solution is 1000g to know the mass of the water substract mass of the acetic acid from...
Tuesday, December 7, 2010 at 12:07pm by Redae
chemistry
The molar mass of acetic acid is 24+4+32=60 Then, There is 0.201 mol acetic acid per litre or 0.201*60=12.06g of acetic acid The density is 1g/ml to change to g/l it becomes 1000g/l then the solution is 1000g to know the mass of the water substract mass of the acetic acid from...
Tuesday, December 7, 2010 at 12:07pm by Redae
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
chemistry
if 1.5g of salicylic acid is heated with an excess of acetic anhydride, what is the theoretical yield of acetylsalicylic acid?
Tuesday, January 4, 2011 at 8:17pm by kelis
chemistry
#2 is the incorrect one. SO2 is the anhydride of H2SO3; SO3 is the anhydride of H2SO4.
Monday, October 1, 2012 at 8:18pm by DrBob222
Chemistry
Do you have a density? 0.67275 M = 0.67275 moles acetic acid/L soln. That is 0.67275 moles x molar mass acetic acid = grams acetic acid = ?? mass = volume x density; convert g acetic acid to volume acetic acid. And that is mL acetic acid/1000 mL soln. Convert that to mL acetic...
Monday, October 25, 2010 at 5:12pm by DrBob222
chemistry
Assume you used 0.200g of salicylic acid and 0.480mL of acetic anhydride, and you obtain 0.152g of pure, recrystallized, dry aspirin. Calculate the percent yield.
Sunday, January 27, 2013 at 8:14pm by Mec
chemistry
Calculate the number of moles in each of the following: 0.150 g of salicylic acid 0.30 mL of acetic anhydride (density = 1.08 g/mL)
Friday, February 24, 2012 at 8:46am by Pat
chemistry
If you use 1 gram of salacylic acid and 3ml of acetic anhydride & 3 drops of phosphoric acid and 1 ml of water after boiling = 0.55 g of aspirin. What is the % yield?
Friday, June 1, 2012 at 7:43am by rachel
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
Ochem
In the reaction between p-aminophenol and acetic anhydride to form acetaminophen, what was the purpose of adding water to the reaction mixture? There are a couple of possible answers, and this requires a detailed explanation for credit. thanks!
Saturday, March 10, 2012 at 12:50am by chi
Chemistry
Calculate the theoretical yield of aspirin to be obtained in this experiment, starting with 2.0 g of salicylic acid and 5.0 ml of acetic acid anhydride (density = 1.08 g/ml).
Sunday, April 20, 2008 at 5:53pm by Sara
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
HAc + NaOH ==> NaAc + H2O so it is a 1:1 titration mixture. Therefore, mLacid x M acid = mL base x M base. Substitute and solve for the one unknown. B) Determine moles acetic acid, then grams. moles = M x L grams = moles x molar mass %acetic acid = (grams acetic acid/...
Thursday, October 20, 2011 at 12:29pm by DrBob222
chem
if you were to react 14.00 grams of salicylic acid with 8.50 grams of acetic anhydride, what would your theoretical yield be? the reaction is C7H6O3+C4H6O3--> C9H8O4 + C2H4O2 assuming 1:1 ratio.
Tuesday, September 1, 2009 at 3:51pm by lyne
chemistry
If you used 0.155 mL of acetic anhydride, and 0.165 g of p-aminophenol what was your theoretical yield of acetaminophen? ___________g If you recovered 0.173 g of acetaminophen, what was your percent yield? ________%
Wednesday, October 19, 2011 at 1:47am by ej
Chemistry
1. Isolation of aniline by steam distillation. (a) Why is NaOH added before performing thedistillation? (b) Suggest a reason for the milky appearance of the distillate and for the change in appearance upon addition of HCl. After having isolated the reduction product, aniline, ...
Thursday, October 19, 2006 at 8:58pm by Lindz
chemistry
My assumption, when you say 5.88% by volume that you mean 5.88% v/v or 5.88 mL acetic acid/100 mL solution. If that is so, then each mL solution contains 0.0588 mL acetic acid. mass = volume x density so mass = 0.0588 mL x 1.049 g/mL = ?? Change that to moles. moles = g/molar ...
Tuesday, September 15, 2009 at 2:08pm by DrBob222
Chemistry
You CAN use the answer from part A but it isn't necessary. moles NaOH = M x L moles vinegar = moles NaOH moles = grams vinegar/molar mass vinegar and solve for grams. Then % acetic acid = (mass acetic acid/mass sample)*100 = ?? You will need to use the density information ...
Sunday, April 3, 2011 at 2:25pm by DrBob222
Chemistry
A solution of vinegar is 4.96% by mass acetic acid in water. Assume the density of the solution is 1g/mL. What is the pH? I have calculated the molar mass of acetic acid to be 60.5
Saturday, April 24, 2010 at 12:24am by Mike
chemistry
Can somebody point out the step i have to take to solve this problem. It would be much appreciated. Thanks a lot!!!! _____________________________________________________________________________________________________________________ Asprin, C9H8O4, is prepared by reacting ...
Sunday, September 16, 2007 at 8:26pm by manny
chem-acid-base titrations
Acetic acid (HC2H3O2) is an important component of vinegar. A 10.00mL sample of vinegar is titrated with .5052 M NaOH, and 16.88 mL are required to neutralize the acetic acid that is present. a.write a balanced equation for this neutralization reaction b.what is the molarity ...
Monday, April 21, 2008 at 10:06pm by natash
Chemistry
Assuming the density of vinegar is 1.0 g/mL ' what is the molarity of vinegar? (use the percent by mass of acetic acid to vinegar which is 5%.) The molar mass of acetic acid is 60.05 g/mol?
Sunday, April 10, 2011 at 10:26pm by Anonymous
chem.
A 10.0 mL of vinegar, an aqueous solution of acetic acid (HC2H3O2), is titrated with .5062M NaOH, and 16.58mL is required to reach the equivalence point. A. What is the molarity of the acetic acid? B. If the density of the vinegar is 1.006 g/cm^3, what is the mass percent of ...
Friday, March 7, 2008 at 12:33pm by Aditya
Chemistry
Look up the freezing point of benzene, then delta T = f.p.=3.5 = Kf*m Solve for molality. molality = moles/kg solvent Solve for moles. moles acetic acid = grams acetic acid/molar mass acetic acid Solve for molar mass. You would expect to find 60 for the molar mass CH3COOH. You...
Friday, February 17, 2012 at 8:08pm by DrBob222
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
Chemistry
I don't get those numbers. Apparently you are using acetic anhydride as the limiting reagent. Unless I made a goof in my calculations, and I may have done that, salicylic acid is the limiting reagent. If you will show your calculations I can check it better.
Sunday, April 20, 2008 at 5:53pm by DrBob222
Chemistry
5.94 g acetic acid has how many moles. moles = grams/molar mass = ?? moles. There are 6.022E23 molecules acetic acid in 1 mole; therefore, there will be 6.022E23 x # moles = xx molecules in 5.94 g acetic acid. The formula for acetic acid is HC2H3O2 so there are 2 C atoms in 1 ...
Tuesday, November 9, 2010 at 8:19pm by DrBob222
chemistry
I have to find the theoretical yield of acetylsalicylic acid in the exeriment? I used 5.0 mL acetic anhydride which is about 5.40 grams. When I calculated the theoretical yield, I got 9.53 grams. Is this number correct?
Wednesday, April 4, 2012 at 3:08pm by casey
First Year Chemistry
what is the balanced equation involved? (CH3CO)2O + H2O → 2 CH3CO-OH so you have to know how much acetic anhydride you have, convert that to moles, and then you need the same number moles of water.
Sunday, March 11, 2012 at 5:05pm by bobpursley
science
asprin (C9 H8 O4) is produced by the rection between salicylic acid (C7 H6 O3) and acetic anhydride(C4 H6 O3). Calculate the maximum mass of aspirin that can be obtained if you mix 50g of each of the reactants. The chem.equation for the reaction is as f.f C7 H6 O3(s) + C4 H6 ...
Monday, May 9, 2011 at 3:27pm by allan
chemistry
vinegar is 5% acetic acid by mass and has a density of 1.02g/mL.what mass of acetic acid ,in grams, is present in 185 mL of vinegar.
Friday, August 26, 2011 at 8:49pm by marion
chemistry 30a
1. Write the equation and balance it. 2. Use PV = nRT and solve for n = moles CO2. 3. Using the equation #1, convert mols CO2 to moles acetic acid . 4. Convert mols acetic aci to grams. g = moles x molar mass. 5. With grams acetic acid you can go to the solution you have. 6. ...
Monday, March 12, 2012 at 9:14pm by DrBob222
Chemistry
A solution is 40% acetic acid by mass. The density of this solution is 1.049 g/mL. Calcu- late the mass of pure acetic acid in 120 mL of this solution at 20 C.
Sunday, October 10, 2010 at 10:37pm by Eric
chemistry
vinegar is made by adding 33 g of acetic acid to 625 if water what is the percent by mass of acetic acid in this solution of vinigar
Tuesday, February 8, 2011 at 10:55pm by Linda
Chemistry
Dissociation is almost the same as ionization; for example, NaCl in H2O dissociates into Na^+ and Cl^-. Acetic acid ionizes into CH3COOH + H2O ==> H3O^+ + CH3COO^- Association is the reverse of dissociation; i.e., positive and negative ions come together. An example is ...
Saturday, February 2, 2013 at 1:01am by DrBob222
Chemistry
mols NaOH = M x L = 0.150 x 0.0400 = ? mols acetic acid = same as mols NaOH. That gives you mols acetic acid in 3.30 mL. That times molar mass acetic acid gives you grams acetic acid in 3.30 mL. g acetic acid in 3.30 mL x (mL in 1 qt/3.30) = ?
Thursday, June 28, 2012 at 11:24pm by DrBob222
Chemistry
ok on Fe. You mean an anhydride. An anhydride is the anhydrous form (without water) of an acid. So add water to each of the compounds and see which produces an acid. Example, Na2O + H2O ==> NaOH (not balanced). So it can't be choice a.
Sunday, May 31, 2009 at 7:21pm by DrBob222
chemistry
5% w/v means 5 g acetic acid/100 mL soln. mols acetic acid = 5/molar mass acetic acid. volume of soln = 0.1 L M = mols/L soln
Wednesday, October 31, 2012 at 3:12am by DrBob222
chemistry
what is the theoretical value for the M of acetic acid in vinegar if the vinegar is 5% acetic acid by a % mass value. Additional info: the experimental M of the acetic acid in vinegar is 0.80M Thank you!!
Sunday, June 6, 2010 at 3:42pm by stacey
Chemistry
what is the theoretical value for the M of acetic acid in vinegar if the vinegar is 5% acetic acid by a % mass value. Additional info: the experimental M of the acetic acid in vinegar is 0.80M Thank you!!
Sunday, June 6, 2010 at 2:07pm by Lolo
Chemistry
Assuming the mass of 5% Acetic Acid is 1.0g/mL, what volume of acetic acid is required to neutralize 25.0mL of 0.10M NaOH?
Thursday, November 12, 2009 at 8:27pm by EDK
Chemistry
Aspirin (C9H8O4) is synthesized by the reaction of salicylic acid (C7H6O3) with acetic anhydride, C4H6O3. 2C7H6O3 + C4H6O3 −→ 2C9H8O4 + H2O When 19 g of C7H6O3 and 19 g of C4H6O3 react, which is the limiting reagent?
Sunday, September 23, 2012 at 11:57pm by Andrea
CHEMISTRY-Explanation Please
In the laboratory, 3.50 grams of salicylic acid were reacted with 7.20 ml of acetic anhydride (density equal to 1.08 g/ml). Determine the limiting reagent. Calculate the theoretical yield of the product, acetylsalicylic acid (ASA), produced in the above reaction.
Sunday, November 25, 2012 at 9:29pm by Yaw
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