i need a laboratory method to measure the conversion in an esterification reaction?
104161
You could rig a "Dean-Stark Trap" on the side of your condensor. That will eliminate water from your esterification (assuming its similar to the Fisher esterification) and force the production of more water and product, until one of the reagents is used up or an equilibrium is achieved.\n\nAnother method would be TLC, comparing the starting reaction mixture to the final product.\n\nSpectroscopy (NMR, IR) could be used.\n\nFinally, you could just put some of your sample into a GC-MS.
757185
The Lewis or Brønstedt acid-catalyzed esterification of carboxylic acids with alcohols to give esters is a typical reaction in which the products and reactants are in equilibrium.\n\nThe equilibrium may be influenced by either removing one product from the reaction mixture (for example, removal of the water by azeotropic distillation or absorption by molecular sieves) or by employing an excess of one reactant.\n\nIf you want to reverse the equilibrium, add water or remove the alcohol.
754842
thats not so hard... all you have to do is titrate it against an acidic solution of known concentration that has a mole ratio of 1:1with sls. add a indicator ( phenolphthaleine) to find the endpoint and that should do it.
817601
try the local chemist....
125296
use spectrophotometric method(uv-vis spectrometry).Few things u shud remember.....\n1) Use Labert-Beer's law\n2) u shud know the molar extingtion coefficient value of that particular species\n3) concentration of the species\n4) Calculate lambdamax. using LB law\nIt is an indirect method.\n\nUV-VIS. Spectroscopy will give u the lambdamax value directly...alongwith absorbance
144359
If you have the reaction A + B -> C + D, under pseudofirst order conditions where B is in excess assuming a rate law of d[A]/dt = k[A][B] = k(obs)[A], observation of [A] should be a first order exponentional over time.  You can confirm the first order exponentional by plotting ln([A]) vs. time, which should be linear.  If you have some sort of autocatalysis - d[A]/dt = k[A][B][C], then the plot of ln([A]) vs. time will deviate from the linear with a larger deviation as the reaction progresses.  Another possibility other than autocatalysis for the not strictly linear log plot could be a change in the reaction medium as the reaction progresses.  If one of your products - say C - significantly more or less polar than A, you might be changing the rate of your reaction which the changing solvent mixture.
1117999
First make a chemical equation, balance it, and find a mole ratio.  Use that ratio and the above information to solve the problem.
988889
understanding the reaction meachanism \neffect of catalysts etc....\ndetermining the amounts needed
327573
Let's see...it's desireable because it's likely to be a lot different than your starting material and your derivatizing agent - this gives you confidence that you actually made a derivative and are not just measuring the m.p. of either your unreacted agent or your starting material.  We used this a lot when I took a class called the Analysis of Organic Unkowns.  No instruments were allowed.
84780
!!!!!!!!!!!!!!!! \nI think rather u wanted to ask how can u predict the formula of a chemical reaction!!\nFirstly, we have to determine the moles of reactant taking part.(It can be done easily, think A reacts with B, just mix 1 mole of A with the same amount of B.)\nThen determine what are the different products and their amounts.\nAll u have to do is some calculations..................\nRemember its not as easy as it sounds.
715055
First off, you need the concentration of the NaOH solution.  From that you can determine the number of moles of NaOH that were used.  This is equal to volume (V) time the concentration, in mol/L (C).\nn = V * C = 0.02260 L * ? mol/L = ? mol\nn = 0.02200 L * ? mol/L = ? mol\n\nThe reaction of KHP (C8H5O4K) and NaOH is this:\nHOOC-C6H4-COOK + NaOH -> NaOOC-C6H4-COOK + H2O\nSo, 1 mol of NaOH will react with 1 mol of KHP.\nThat means that the number of moles of NaOH you calculated above is also equal to the number of moles of KHP.\nThe molecular weight of KHP is 12*8 + 1*5 + 16*4 + 39 = 204 g/mol\nMultiply that by the number of moles: 204 g/mol * ? mol = g actual KHP\n\nYou can divide that number by the 0.911 and 0.950 g and then multiply by 100% to find the purity.\n\nHere’s an example if your NaOH solution was 0.1 M (M means ‘molar,’ or mol/L):\nn = 0.02260 L * 0.1M = 0.002260 mol of NaOH = 0.002260 mol of KHP\n204 g/mol * 0.002260 mol of KHP = 0.461 g pure KHP\n0.461 g pure KHP / 0.911 g impure KHP * 100% = 50.6 % KHP\n\nHope this helps!
173108
There will be no easy or fast way.  Some options:\n\nhttp://www.analoxusa.com/frame120tb.htm\n\nchemistry.uca.edu/Projects/Quant98/urea-ise-98.pdf \n\nhttp://biocompare.com/newtech/1522/QuantiChrom(tm)-Urea-Assay-Kit.html\n\nwww.springerlink.com/index/X07825U10H247238.pdf
955797
Use the Arrhenius equation to predict the rate:\n\nhttp://en.wikipedia.org/wiki/Arrhenius_equation\n\nK = Ae -E/RT\n\nIt all boils down to your reactants, the activation of energy, and the product that is being synthesized.
724819
To determine the concentration of a reagent.
900972
You could use a turbidometric method that could detect the diffraction of light through the liquid and correlate it with the amount of microbial growth in it.  \n\nYou could also use a calibrated loop to plate the liquid and then count colonies.  I know they do this with urine cultures in hospital labs at times.  The loop picks up a certain amount of liquid like 10 microliters or so and then you can correlate the growth with this 10 microliter figure.
481495
1. Perform vacuum distillation.  Place the solution in a vacuum flask; apply vacuum (removing air from vessel); apply heat and "boil" the water off.  Collect the condensate and measure its volume.  Weigh the remaining sugar that is left behind in the vacuum flask.\n  -or -\n2. There may be a way to measure the refractive index of the sugar solution.\n-or-\n3. Heat a sample of the solution to determine the boiling point elevation; if you have a table that compares molarity vs. boiling point elevation, you may be able to determine the molarity of the solution by knowing at what temp. the solution boils.\n\n4. You may be able to extrapolate by weighing exactly one cubic centimeter (cc) (volume) of the solution at 25 degrees C.  There may be a table comparing weight of a 1 cc solution at that temp (as the density of 1 cc of water is different than a 1cc sugar solution.
188870
a scale or balence that uses grams