reaction of polymer with Sodium Carbonate
121940
There are thousands of polymers all with very different chemical and physical properties.  so a simple answer can not be given.  perhaps a specific polymer would obtain better responses.
326527
See if these help\n\nhttp://www.pslc.ws/macrog.htm\n\nhttp://www-classes.usc.edu/engr/ms/125/MDA125/polymers_files/frame.htm
622656
Na2CO3 + 2HCl-> NaCl + H2O + CO2
547785
The size of the ion is an important consideration. K+ is bigger than Na +.\n\nIn ion exchange operation, sodium is the most common ion to "slip" from the resin.
270734
Benzene and magnesium hydroxide and magnesium bromide.\n\nI am betting you are doing a Grignard reaction\n\nEthyl benzoate + 2 phenylmagnesium bromide --> triphenylmethanol•MgBr salt\n\nif water is present, the grignard reacts with the water first\n\nPhenylmagnesium bromide + H2O --> benzene + MgOHBr
123232
First of all, you're a nut.  Or at least a guy who likes to buy new microwaves.\n\nI'm not sure there is an actual reaction between sodium hydroxide and sugar.  For the sake of chemistry, we can treat all sugar as C6H12O6.  If anything the reaction will produce carbon dioxide and water, but this happens anyway when you burn any sugar so it might be hard to separate the two processes. \n\nWill check and get back to you  :)\n\nUpdate:  See the link below.  The only thing I can find is that NaOH will oxidize glucose, though this doesn't work as well for sucrose.  I don't think heating will have any effect other than to make the reaction go faster (and it already goes pretty fast, apparently.\n\nHave you thought about a career in chemistry?  You have the right kind of mind for it -- i.e., let's throw these chemicals together and see what happens!  By the way, I would NOT try this with NaOH and any kind of acid solution.  It might be dangerous under the wrong conditions.
646536
Are you preparing a buffer soln with NaHCO3 and NaCl ? Then take equimolar amounts of both and dissolve them in 100 ml of water and then dilute them to the desired strength.
516189
The answer will depend on th strength of the solution. At an equal concentration,  sodium hydroxide will have a much higher pH than an solution of sodium carbonate.\n\nA 10% solution of sodium carbonate will have a much higher pH than 0.00001 M solution of sodium hydroxide.
350439
This synthesis reaction would produce NaBr(s).\n\nOh, I noticed that your choice for 'systhesis' reaction was 'formation'.  Means the same thing.
479683
A thorough perusal of your textbook should help with your problem.  Oh, wait--sorry, I forgot--you aren't interested in LEARNING how to calculate the pH of your sodium acetate solution, just in getting the quick fix answer from someone who has.
184868
There should be no reaction.  Sodium bicarbonate is very weak base and will only hydrolyse methyl/ethyl esters very very slowly or help dissolve carboxylic acids in aqueous media. \n\nThere are no protons acidic enough on cinnamaldehyde for the two to react together.
372917
2 Na (s) + 2 H2O (l) --> 2 NaOH (aq) + H2 (g)\n\nThe metallic Sodium is being oxidized and is the reducing agent.\n\nPotassium has a lower ionization potential than Sodium and so tends to react faster.
18255
3AgC2H3O2 + Na3PO4 -----> Ag3PO4 + 3NaC2H3O2
288263
NaHCO3(s) + CH3COOH(aq) → CH3COONa(aq) + CO2(g) + H2O(l) \nThis is the real chemical reaction.
118604
Well i can't paste that on here for you...but consult this link; http://www.abb.com/GLOBAL/NOOFS/noofs187.nsf/viewunid/713C646EB0A24CCBC12569EE0036977F/$file/PS.pdf#search='MAKING%20POLYSTYRENE%2C%20process%20flow%20diagram'\n\nIf u can't access via the above link, go to http://www.search.abb.com Then type 'making polystyrene' or :PS Web 2001" Folow the first link...its a pdf file.
374810
Na2CO3 + 2HNO3 → 2NaNO3 + H2O + CO2\n\n0.1L * 0.2 mol/L = 0.02 mol HNO3\n\n0.02 mole HNO3 * 1 mol CO2/2 mol HNO3 = 0.01 mol CO2\n\nNow plug 0.01 mol CO2 into PV=nRT, using STP conditions.\n\nPV=nRT\n\nV = nRT/P\n\nV = (0.01)(.0821)(298)/(1)\n\nV = 0.24 L\n\n\n*** The person above me did it WRONG!  He confused sodium carbonate with sodium bicarbonate.  Also, he completely forgot to do the stoichiometric conversions.  He solved for moles of HNO3, and then plugged it into PV=nRT.  You must first convert moles of HNO3 to moles of CO2 with stoichiometric conversions, using the BALANCED equation.
526487
Without knowing exactly what you did I can't answer this question!  Dissolution in dilute sodium hydroxide solution, filtration to remove any fillers etc, re-precipitation with hydrochloric acid and isolation by filtration should have given you an answer of some sort. Not exactly accurate though.