What is the diffrence between Mohr , Wolhard , Fajan  titration?
831078
Mohr- formation of second colored precipitate\nuseful pH range 7-10\n\nVolhard- Formation of colored complex not precipitate\n\nFajan Titration- Colored absorbed species formation\nlimited to precipitation reactions leading to colloids
528995
Hmmm, what exactly do you mean by INSTRUMENTAL techniques? As the guy before me said, you could titrate it against a strong coloured oxidising agent such as acidifies potassium permanganate. But you can't really get the concentration from a spectrophotometer, for example, since peroxide (H2O2) doesn't absorb light.\nI guess you could thry using a NMR spectrometer for the job, or some kind of chromatography, but titration is by far the safest and easyest.
697747
Hydroxy Naphthol Blue as a metallochromic indicator can be used  in the chelometric titration.
760435
You are looking at a displacement reaction, in which the more reactive metal (Cu) is displacing the less reactive metal (Ag) from its salt solution (AgNO3).\nCu (s) + 2AgNO3 (aq) --> 2Ag (s) + Cu(NO3)2 (aq)\n\nHope this helps. :)
526021
Molisch's Test is the reaction of 1-naphthol with carbohydrates in the presence of sulfuric acid.  Carbohydrates are oxidized in this system to furfural derivatives, which will condense with the naphthol to give a purple-colored dye.\n\nFehling's Test is for aldehydes.  Copper (II) sulfate and Rochelle's salt (potassium sodium tartrate) solutions are combined, which causes complexation of the copper with tartrate.  An aldehyde will reduce the copper (II) to copper (I), which will precipitate as Cu2O, a red solid.  Ketones do not react in this manner.
871220
The second one:\nAF + H --> AFM + TM\n\nActivation E: +10KJ/mol is moderate\nHeat of Rx= +5.2 KJ/mol is positive, making this an endothermic reaction (requires the input of heat or energy to accomplish).\n\nSee the site below:
462489
put one of the acids in the titer, the other in the flask underneath.  Use a magnetic stirrer in the flask to ensure good mixing and ensure that you take required precautions (like goggles gloves lab coat ...possibly in a fume cupboard).\n\nThe two acids don't react with each other but is this 4:1 mix not acqua regia?
1030596
Cr is the concentration of the species, the r (which I assume is subscripted) stands for it being the reduced form, it has no numerical value and is done to better describe the nature of the species.  Co is used for the reverse step of the reaction.
876235
The product of a neutrilization reaction is always water and a salt, so use that as a guide.  For part 2, use the units as a guide.  Hint M=molarity=mols/L
526901
Well, there are two types of hardness I know in chemistry. I don't know which of the two you are referring to so I'll just list both. \n\nThe first one is called "carbonate hardness", commonly known as alkalinity. It is the meaure of the ability of a solution to neutralize acid without changing the pH. It both controls and maintains water pH, and it is measured in degrees (dKH), parts per million of calcium carbonate (ppm CaCo3), or milliequivalents per liter (meq/L).\n\nThen, in contrast to carbonate hardness, there is general hardness which is the measurement of the total dissolved minerals in a solution. Test kits for general hardness measure the amount of calcium and magnesium salts present, and the result is expressed in degrees dH or dGH.
325143
For gold= symbol FCX\nFor silver= symbol WTZ
952788
A=E*d*C\n\n(d=length of the path of the light through the solution)\n\nIf you have only one value of absorbance then obviously there is no way of determining the concentration without the molar extiction coefficient (E).\n\nIn practice even if you know E, you don't use it to find the unknown concentration. Instead you measure the A of standard solutions and do a standard curve. From the equation of that curve (which you find using linear regression) and the value of A of your sample you calculate the unknown amount. \nThe standard curve doesn't need to be A vs mole/lt. It can be A vs anything e.g. g/ml, mg/ml, ppm or even just g, mole, etc. the only thing that changes is what the slope represents.\nFor example for A vs mole/lt the slope corresponds to E*d, for A vs g/lt the slope corresponds to E*d/MW, etc.\n\nIf you  always have the same volume of sample you can do the curve A vs grams directly. Then if V is the volume of the sample, the slope corresponds to E*d*V/MW\n\nEven if your standard curve is expressed in moles/lt you can convert it to grams. You just need the MW of the compound and the volume, not E...
186841
Volumetric Analysis also known as Titration is a standard laboratory method of quantitative/chemical analysis which can be used to determine the concentration of a known reactant. Because volume measurements play a key role in titration, it is also known as volumetric analysis. A reagent, called the titrant, of known concentration (a standard solution) and volume is used to react with a measured volume of reactant (Analyte). Using a calibrated burette to add the titrant, it is possible to determine the exact amount that has been consumed when the endpoint is reached. The endpoint is the point at which the titration is stopped. This is classically a point at which the number of moles of titrant is equal to the number of moles of analyte, or some multiple thereof (as in di- or tri- protic acids). In the classic strong acid-strong base titration the endpoint of a titration is when the pH of the reactant is just about equal to 7, and often when the solution permanently changes color due to an indicator. There are however many different types of titrations.\n\nMany methods can be used to indicate the endpoint of a reaction; titrations often use visual indicators (the reactant mixture changes colour). In simple acid-base titrations a pH indicator may be used, such as phenolphthalein, which turns (and stays) pink when a certain pH is reached or exceeded. Due to the logarithmic nature of the pH curve, the transitions are generally extremely sharp, and thus a single drop of titrant just before the endpoint can increase the pH by several points - leading to an immediate colour change in the indicator. That said, there is a slight difference between the change in indicator color and the actual equivalence point of the titration. This error is referred to as an indicator error, and it is indeterminate.\n\nEtymology\nThe word "titration" comes from the Latin "titalus," meaning inscription or title. The French word, titre, also comes from this origin, meaning rank. Titration is by definition the determination of rank or concentration of a solution, so it corresponds.\n\nPreparing a sample for titration\nTitrations are performed "in solution". If the sample isn't a liquid or solution the samples must be solved. If the analyte is very concentrated in the sample it might be useful to dilute the sample.\n\nAlthough the vast majority of titrations are carried out in aqueous solution, other solvents such as glacial acetic acid or ethanol (in petrochemistry) are used for special purposes.\n\nA measured amount of the sample can be given in the flask and then be solved or diluted. The mathematical result of the titration can be calculated directly with the measured amount. Sometimes the sample is solved or diluted beforehand and a measured amount of the solution is used for titration. In this case the solving or diluting must be done accurately with a known coefficient because the mathematical result of the titration must be multiplied with this factor.\n\nA lot of titrations require buffering to maintain a certain pH for the reaction. Therefore buffer solutions are added to the reactant solution in the flask.\n\nSome titrations require "masking" of a certain ion. This can be necessary when two reactants in the sample would react with the titrant and only one of them must be analysed. Or when the reaction would be disturbed or inhibited by this ion. In this case another solution is added to the sample which "masks" the unwanted ion (for instance by a weak binding with it or even forming a solid insoluble substance with it).\n\nSome redox reactions may require heating the solution with the sample and titration while the solution is still hot (to increase the reaction rate).\n\nProcedure\nN.B. Before starting, make sure that all of your glassware—especially the burette—is clean and dry. Alternatively, you can rinse out the glassware with the solution that is to be stored in the particular piece
727505
1. M1X1 (no subscripts), because alkali metals are +1 and halogens -1.\n2. M2X1 (subscript 2 for the metal), because group 6a elements are -2 in binary compounds\n3. MX2, because alkaline earths are +2.\n4. MX (subscripts each 1) because alkaline earths are +2 and group 6a elements -2.\n5. MX3, because group 3a metals are mostly +3. An important exception is thallium, which is either +3 or +1. So thallium chloride could be TlCl or TlCl3.
284075
It's fairly easy don't worry.\n\nNo need for d level splitting diagrams to answer this since we're dealing with N and F:  use the spectrochemical series to make an assumption about the ligand.  The difference in t2g and eg levels (∆o) determines whether a complex is low or high spin.  If both ligands were the same, we would have to look at the oxidation state of the ligand in the complex.\n\nHalides <  Oxygen ligands  <  Nitrogen ligands < CN- ligands\n\n   ALWAYS HIGH SPIN    ---------------            ALWAYS LOW SPIN\n\nIf ∆o > P, then a complex is low spin.  IF ∆o < P the complex is high spin.
225634
None. They are two different compounds.\n\nIt looks like you want to compare a specific property of the alcohols. Please specify!
383531
========\n\nApparently purity, calculation or measurement errors have been there.\n\nYou repeated the thrice from the same solution to get an average.\n\nTry another solution.