what kind of water must be used for chemical analysis purposes?
111661
there are different levels of purity of water and other solvents. the more pure the solvent is the more expensive.\nfor most introductory labs or where the results aren't critical then walmart quality distilled or deionized water is ok.\nfor other purposes you'd want to use the really good stuff.
546593
Water that is ionized?¿?
50776
hydrogen, oxergen, minerals, baceria... depends what water your drinkig.
752263
titration is a very useful method for: pharmaceutical analysis, food analysis, oil analysis, pollution and environmental analysis. so users can be Chemists and Chemist engineers.
1123940
Hard Water--\nHard water is water that has a high mineral content (water with a low mineral content is known as soft water). This content usually consists of high levels of metal ions, mainly calcium (Ca) and magnesium (Mg) in the form of carbonates, but may include several other metals as well as bicarbonates and sulfates. While it is not generally dangerous to safety or health, it does generally cause potentially costly nuisance problems in the home and in industry. On the other hand, hard water is considered to be ideal for brewing certain styles of beer. Kentucky's distinctive Bourbon whiskey owes its flavor in part to the high calcium content of its groundwater (compared to the pilsener style of beer, the brewing of which requires very soft water). Some hard water chemicals, particularly silicates and calcium carbonate, are also effective corrosion inhibitors, and can prevent damage to pipes or contamination by potentially toxic corrosion products.\n\nThe simplest way to determine if water is hard or soft is the lather/froth test. If the water is very soft, soap will tend to lather up easily when agitated, whereas with hard water it will not. Toothpaste will also not froth well in hard water. More exact methods of hardness detection use a wet titration method to determine hardness
628336
as opposed to polluted water?
924300
The best thing to use is a water filter. They get rid of temporary hardness that causes scale, along with chlorine, lead, aluminium, and other trace metals. However, they do not purify water, best to buy a packet of water purifiers from the chemist.
7198
You may wish to try abe.com.  I am a librarian and I occasionally source texts from abe.com, alas with the title you provided there is nothing available.  I also checked alibris.com but they had no copies. \n\nI also checked WorldCat, a union catalog for thousands of libraries worldwide and I found no holdings with that exact title.  There was one called <<Standards of drinking water quality and methods of examination applicable to European countries; report on a study.>>\nAlso available in WorldCat was <<Standard Methods for the Examination of Water Sewage and Industrial Wastes>>. \n\nYou may wish to make certain the title is correct, also providing an author would help.  \n\nWorldCat is a fee based database which your librian can access for you or help you access on your own. \n\nGood luck.
1043394
Of course you must specify whether you want the thermodynamic properties of water (or chewing gum?).  Good luck.
417834
Something that requires water in order to become a true Base\n\ne.g. CaO + H2O -> Ca(OH)2
87390
There are several possible answers to this question, depending on what resources you have available to you.  If the solution you are measuring is known to contain only potassium carbonate dissoved in water, you can measure the potassium concentration by either atomic emission or atomic absorption methods and calculate to concentration of the potassium carbonate.  You could measure the carbonate concentration by titration or colormetric methods and calculate the potassium carbonate concentration.  Or you could simply evaporate a known quantity of the water to dryness, weigh the residue and calculate the concentration from those numbers.  \n\nIf you have other compounds in the solution, the last option, gravimetric, pretty much disappears.  The first two options are still practical, unless the other compounds contain potassium or carbonate.  Then, things get a little more complex.
893507
What about the substances USED for water treatment?  If there are effective and safe water treatment, handy substances , that would be ideal to market.  Everyone wants to have their own "substance" to "treat" their water/ if you know what I mean.
129035
Liquid water, by and large, with some dissolved materials.
610466
Spectrophotometric methods, or those based on the absorption of light by an analytical species, are some of the simplest and most common methods used in quantitative analysis. The amount of light which is absorbed by the sample (A) is correlated with the concentration (c) of the analytical species present using Beer's Law (A = e bc; where e is the molar absorptivity for the analytical species and b is the pathlength of the sample cell). \n\nIn this experiment, the analytical species, iron, will be studied using a colorimetric method in which a reagent is added to transform iron into a highly absorbing complex. Iron is often found in nature in reasonably high concentrations and may enter the hydrosphere through the weathering of iron salts and minerals. Both iron (II) and iron (III) ions are commonly found dissolved in water either in a colloidal form or as inorganic or organic complexes. There are also multiple anthropogenic sources of iron in the environment such as canneries, tanneries, textile mills, and metal cleaning operations. \n\nA relatively simple but sensitive colorimetric procedure for the determination of iron involves first reducing all iron present in the sample to iron (II) ion using hydroxylamine hydrochloride and then complexing with 1,10-phenanthroline in a solution buffered at low pH:\n\nPart 1: Preparation of Iron Standard Solutions\n\nWeigh 351 mg of high quality ferrous ammonium sulfate hexahydrate (FeSO4(NH4)2SO4 Ÿ 6H2O) and quantitatively transfer to a 500 mL volumetric flask. Add 50 mL of distilled water followed by 1 mL of concentrated sulfuric acid. Dilute to the mark with distilled water and mix thoroughly. Using this solution, prepare five standard solutions of iron (II) ion (about 10 - 15 mL should be sufficient) ranging in concentration from 0.5 to 5 ppm.\n\nPart 2: Preparing a Beer's Law Plot\n\nTransfer a 5 mL aliquot of the lowest concentration iron standard solution (probably 0.5 ppm) to a 125 mL Erlenmeyer flask and test the pH with test paper. If the pH is greater than 4.5, add enough 0.2 M sulfuric acid to bring the pH to about 3.5, counting the number of drops that you have added. \n\nAgain, counting the drops that you add, add sodium citrate (259 g/L) buffer to bring the pH to about 4.5. Pipet 1 mL of 10% hydroxylamine hydrochloride and 3 mL of 0.3% 1,10-phenanthroline into the sample and mix the solution well. Allow about 5 min for development of color.\n\nUse the same number of drops of sulfuric acid and sodium citrate for your remaining standard solutions. For each solution, add 1 mL of 10% hydroxylamine hydrochloride and 3 mL of 0.3% 1,10 phenanthroline and mix the solutions well. Allow about 5 min for development of color for each solution.\n\nScan the absorbance of each of the solutions from 300 to 600 nm using the Shimadzu ultraviolet-visible spectrometer, noting the absorbance value of each solution at 510 nm. For each sample, use water as your reference blank.\n\nPart 3: Analysis of samples\n\nWater samples should be measured for each member of your group in addition to determining the iron concentration in an unknown water sample provided by the Instructor. Treat the samples in the same way as the standards: using a 5 mL sample, add sulfuric acid initially, if necessary, to adjust the pH, followed by citrate buffer, reducing agent (1 mL of 10% hydroxylamine hydrochloride), and the indicator (3 mL of 0.3% 1,10 phenanthroline). Mix the solutions well and allow about 5 minutes for development of the complex. \n\nScan the absorbance of each of your sample solutions from 300 to 600 nm using the Shimadzu ultraviolet-visible spectrometer, noting the absorbance value of each solution at 510 nm. Using your Beer's Law plots prepared in Part 2 and the measured absorbances of your samples, determine the iron concentrations in each of your water samples.
108125
The problem with using distilled water is the local carbon dioxide in the air.  This CO2 will instanly mix with the water, and moreso over time, creating carbonic acid in the water, lowering its resistance.\n\nYou really need DEIONIZED water and keep it in a closed system made of plastic which will prevent gas transfer or ions from collecting in the water.  Then you dispense the water from a valve or something right at the point of use, to avoid CO2 contamination.  DI filters are commonly used in laser water cooling systems.  They aren't cheap, but you can buy the housing and filter elements.  You should be looking for 1Mohm or greater for your water supply.
619546
It will of course depend on the rock.  Trace elements could almost be anything.  Look up the minerals involved in your case.  It will also depend on the source of the water.\n\nhttp://mineral.galleries.com/minerals/physical.htm#phy\n\nhttp://webmineral.com/
1035950
The basic check is: measure the mass, divide by the volume of water displaced, check that the density is correct. After that you should still do a chemical analysis to make sure there aren't other heavy metals, like uranium or lead mixed in.