are there any reports of completed science projects using red cabbage and water to determine acids and bases?
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that is plagiarism, and it is illegal. Especially if you are a student, you can be expelled. Do your own work, all other chemists have done their own, now it's your turn.
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There are several uses for this.  Generally for chemistry students the effort teaches them how the measurements are made, good laboratory techniques, and hopefully, some insight into chemistry and the physical sciences.  It doesn't always work, but it makes a good experiment. \n\nFor those who are in the business of using various substances, it is very important to know what their physical properties are, and how they relate to the physical properties of other substances.  Your air conditioner was designed around those measurements, as was your car, paint, furnace, and just about everything that was manufactured around you.  \n\nWhile nature obviously doesn't carefully record properties in a lab book, they are important to how plants and animals work, how hard rocks are, how ice forms, etc.  Without understanding these properties, we can't understand nature or ourselves completely.
766824
My daughter did a project where she tested the absorption of various brands of paper towels.  She did an experiment and wrote a paper on what makes paper towels hold liquids.
1034146
If you're thinking of the natural indicator in red cabbage, it is pink-red under acid conditions, blue-purple under neutral conditions, and greenish yellow under basic conditions.  \n\nSo, with lemon juice (citric acid) it should be red.
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.
1056970
some basic experiments in chem r making of common salt ,mixing hcl with various chemicals 2 produce gases
1005673
test tube- observing for chemical reations
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http://www.scienceaid.co.uk/titration.html
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How about visiting this site:\n\nhttp://www.all-science-fair-projects.com/category0.html
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Not cabbage! The SPECIFIC indicator used is 2,6-dichlorophenylindophenol (DCPIP) - a blue/purple dye reduced by ascorbic aid to it's colourless form. There is no suitable substitute that I know of, although red cabbage extract is an excellent GENERAL acid/ base indicator. \nIncidently the DCPIP method is useless at determining the Vit C content of blackcurrant juice!
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It's good to discover science, but it's important to know what you're doing because some experiments can be dangerous or even fatal.\n\nSome acids, like vinegar and lemon juice, are safe, but other, stronger acids can cause serious injury.
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Vinegar is an acid (Acetic Acid) and baking soda is a base (Sodium Bicarbonate). Mixing acids with bases produces what is called "Acid Reduction Oxidation," or "Redox" reactions. Its basic forms result in salt (the type of salt is dependent upon the mixed chemicals), water, and heat (left over from the reaction). In the case of more complex reactions, where there is enough heat to separate some of the salt compounds, gases such as carbon-dioxide may alo be formed. \n\nThis is what creates the bubbles found in your "volcano."
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I can only tell you the empirical formula of Vitamin C\n\nVitamin C (ascorbic acid) contains 40.92 % C, 4.58 % H, and 54.50 % O, by mass. The experimentally determined molecular mass is 176 amu. What is the empirical and chemical formula for ascorbic acid?\n\nIn 100 grams of ascorbic acid we would have: \n\n40.92 grams C \n\n4.58 grams H \n\n54.50 grams O\n\nI've gone through with those science fair projects.  I suggest that you should present something that could help the environment.  Like my project way back,  I made a fuel cell car.  The car will run bcoz of water not bcoz of gasoline... the process is done through using solar cells.  I decided to have such a simple design and there are lots of sunlight here in our country.  \n\nThough my project seems to be everywhere now with major inventions,  I just presented my own angle of invention, like a simplified one.  \n\nWith your other questions, I'm not familiar with it. Is it something to do with like that of electrical engineering... spinning around or stuff?  \n\nSo, I advice you to have a practical science fair project and since you are in tenth grade, is it something to do with phyiscs?  Out of the world inventions is far beyond... you are still a student but if you want to ba an inventor someday, maybe this is the chance to search and search and search.\n\nMy suggestions,\n\nLook and seek help to your friends, family, inventor (if possible), teacher, etc.  Read books of your interest and concentrate to a project you really want to.  Of course, list all possible projects you like, pros and cons, practicality, and of course, wise spending and safety.  You shouldn't think that you must win the first priwe, all you have to do is to persevere, be determined, think something unique and try to (if ever) look on other work of your competitors... maybe it might help on some idea. \n\nWell, those suggestions are taken from my own experience.  I didn't take any competitons though and it is a requirement.\n\nI guess I take this so long. Good Luck!  I hope I somewhat help you.
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Specifically: water, pyridine, squalene, urea, acetic acid, lactic acid, complex alcohols and glycols, ketones, and aldehydes.
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sciencelab.com has just about anything you'll need!\nhttp://www.sciencelab.com/search.php?q=acetic+acid+-acemetacin+-acetamide+-benzyl
362008
vinegar and baking soda. \nWill also be fun experiment for them!
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Any acid, for example:\n\nHCl + H2O  --> Cl- + H3O+