Hi everybody.I'm writing a homework "Applications of neutralization titrations" and I have no materials .Help!
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http://www.sbuniv.edu/~ggray/CHE3345/chp14.html\nhttp://web.odu.edu/sci/tisenhou/chem321/chap12/index.htm\n\nbest luck
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We have no idea what data you [we] have to work with here.\n\nWhat did you do in your lab?\n\nI assume you had a saturated solution of Ca(OH)2 which you then titrated with a stron acid like HCl.  You then should have recored the volume and concentration of the acid required to neutralize the Calcium Hydroxide.\n\nWrite out the chemical reaction between Ca(OH)2 and your acid, find the mole ratio between the moles of acid used and the moles of OH- in solution, and solve.
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KCl(aq) + AgNO3(aq)  --> KNO3(aq) + AgCl(s)\n\nNet ionic: Cl-(aq) + Ag+(aq)  --> AgCl(s)\n\nNa2SO4(aq) + Ba(NO3)2  --> 2NaNO3(aq) + BaSO4(s)\n\nnet ionic: SO4(-2)(aq) + Ba(+2)(aq)  --> BaSO4(s)
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You might want to try to re-read the questions.  You don't appear to be understanding what is written there.  (I call it a brain fart, but three out of 28 indicates a little lack of understanding)\n\nIf you have re-read the problems, then I offer the below:\n\nYou might want to go over your notes about what a mole is.  It is an amount and a number.  It is a fundamental conceptual building block for the study of chemistry.\n\n  It looks like you expect to be able to plug and chug on these.  Which you can, once you start thinking in terms of atoms and molecules.  Plugging and chugging BEFORE you understand what these little pieces are doing is a recipe for a C.\nIt IS the ATOMIC theory of matter, don't you know.\n\nSo, once you've absorbed that, re-read these three problems.\n\nStill no joy?  Read on, Gunga DIn\n\nFirst H(g) is NOT the element's standard state! I thought everybody learned in grade school about H2 gas - the simplest molecule?  Iodine, I leave to you  (hint a gas???!!! not)\n\nSecond lets see you're making umpteen moles of something and calculate the dS.  that was not the question.  (hint: something about ONE mole)\n\nThird read the problem. your chemical equation is from I don't know where but not from what is in the problem. (hint: products on the LEFT???)
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You might want to go here Protonic (see link below)\n\nThey would help you, is free also.
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This might help :)\nhttp://www.chemicalforums.com/index.php?board=8;action=display;threadid=3263
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The neutralization reaction:\n2NaOH + H2SO4 ---> 2H20 + Na2SO4\nTwo moles of NaOH are required for each mole of H2SO4. \n\nMultiply the molarity and volume (in liters) of the NaOH to find the original number of moles: \n.0346 L * .200 M = .00692 moles NaOH\n\nDivide moles of NaOH by two to get the number of moles of H2SO4:\n.00692 moles NaOH /2=.00346 moles H2SO4\n\nTo find the concentration of sulfuric acid, divide the moles by the volume in liters: \n.00346 moles H2SO4 / .0500 L = .0692 M
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1) FIND THE REDOX-REACTION\n\nChromate (+VI) is reduced to 2 Cr(III) meaning this that 6 electrons are needed.\n\nThe corresponding oxidation on the alpha-C-atom in Ethanol goes from oxidation-level (-I) to oxidation-level (+III) in acetic acid, meaning it delivers 4 electrons per molecule.\n\nSo we find a stochiometric electron equilibrium if 12 electrons are exchanged:\n\n2 Cr2O7(2-) + 3 CH3CH2OH  =  4 Cr(3+) + 3 CH3COOH\n\n2) THE PROCESS MUST BE ELECTRICALLY NEUTRAL\n\nWe add the K-Ions having the left side of the equation neutral and the right side with 16 loads positive:\n\n2 K2Cr2O7 + 3 CH3CH2OH  = 4 Cr(3+) + 4 K(+) + 3 CH3COOH\n\nIn order to have the left side also with 16 loads positive, we add 16 protons, meaning this, that the reaction needs acid. Since we use sulfuric acid we also add 8 sulfat-ions on both sides and hereby can neutralize the product side:\n\n2 K2Cr2O7 + 8 H2SO4 + 3 CH3CH2OH  =\n                         2 Cr2(SO4)3 + 2 K2SO4 + 3 CH3COOH\n\n3) STOCHIOMETRIC BALANCE OF THE ELEMENTS H and O\n\nTaking into consideration that unused protons finally end up as water, we add on the right side 11 H2O and hereby is also reached the balance of oxigen:\n\n2 K2Cr2O7 + 8 H2SO4 + 3 CH3CH2OH  =\n                  2 Cr2(SO4)3 + 2 K2SO4 + 3 CH3COOH + 11 H2O\n\nSo now good luck for counting the atoms!
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Try this paper ...\nhttp://www.citebase.org/fulltext?format=application%2Fpdf&identifier=oai%3AarXiv.org%3Anucl-th%2F0403083
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If you have the letter names, use the Periodic Table of Elements.  If not, use PH paper, and that might help.  Go by color, soluability, and texture.
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use a potato and two different metals as electrodes. The link will help you, do your own homework, or web searching atleast! it was the second link in google for g** sake!
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Links at\n\nhttp://www.itt.edu/staff/boyter/links/index.html#CHEMISTRY_CHROMATOGRAPHY
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Congrats, I am working on my thesis too.  There is PDA (potato dextrose agar), V8 agar (made from guess what, V8) and many others.  Each is designed for a specific purpose.  I am not an expert on this, but try a search engine.
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check this link-- http://www.orgsyn.org/orgsyn/prep.asp?prep=cv6p0468.\n\ninstead of Me use Ph
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Wow, I hope these are right.  I wish i had a solubility chart or something (Which you probably have)  \n\nCuSO4(aq) + Na2S(aq) ---> CuS (s) + NaSO4 (aq)\nNet ionic - Cu2+ (aq) + S2- (aq)  ---> CuS (s)\n\nNiCl2 + 2KNO3 --> Ni(NO3)2 (aq) + 2KCl (aq)\nnet ionic - none (if NiCl2 isn't aq, then this is wrong)\n\nCa(OH)2 + 2HC2H3O2 ---> Ca(C2H3O2)2 (aq) + 2H2O (l) \nnet ionic - H+ (aq) + OH-(aq) ---> H2O (l)\nactually, since the acetic acid is a weak acid, this might be a little different.  If you learned it this way, then your net ionic is:\nHC2H3O2 (aq) + OH- (aq) ---> H2O (l) + C2H3O2- (aq)\n\nHope this helped
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we know that pH is ranged from totally basic to totally acidic, with neutrality (water) being at pH=7; so just display a range from 0 to 14 and color code it (red for acid and blue for basic) and place your findings there (ie before and after situations of NaCl towards the pH of the solution). Also place analogies (ie. the results of the pH due to NaCl concentration of 10% is equivalent to household ammonia)\n\nWhen explaining something to a non-science person, visuals and analogies always helps.
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1.) do your own homework\n2.) this is the computer forum, not high-school chemistry.  Next time post to the right furom.