what are the chemical properties of nitrophenol phosphate and what is it used for?
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The molecular formula is C6H5NO5P\n\nStructure (if in case you want it too) is as follows:\n\nDraw a benzene ring (phenyl group) minus 1 hydrogen (C6H5). To the Carbon without the hydrogen, attach a Hydroxyl group (-OH). \n\nOn the other Carbon positions, whether it is the ortho positions, meta positions, or para position, erase the hydrogen and attach a nitrate group (-NO2). \n\nOn the Oxygen with the double bond to Nitrogen on the Nitrate group, erase one of the bonds and attach this bond to the phosphate group (-PO3).\n\n4-nitrophenol phosphate is used in a substrate for a timed test for alkaline phosphatase turning colors for 4-nitrophenol
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http://www.olysun.com/Chem_121/Soln.html\n\n\ncc
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chemical properties:  high electro negativity\nphysical properties:  it's a halogen
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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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Technical applications\nAlthough NO has relatively few industrial uses, it is produced on a massive scale as an intermediate in the Ostwald process for the synthesis of nitric acid from ammonia. In 2005, the US alone produced 6M metric tonnes of nitric acid. As a raw material it is used in the semiconductor industry for various processes. In one of its applications it is used along with nitrous oxide to form oxynitride gates in CMOS devices.\n Miscellaneous applications\nNitric oxide can be used for detecting surface radicals on polymers. Quenching of surface radicals with nitric oxide results in incorporation of nitrogen, which can be quantified by means of X-ray photoelectron spectroscopy.
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http://chemistry.about.com/library/weekly/blsapon.htm\n\n\n\nSimple web search
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NKP is what fertilizers claim as active ingredients.\n\nNitrates, Potassium, and Phosphates
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http://en.wikipedia.org/wiki/Nitrous_oxide
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P3(NO3)3 \n\nNO3 = nitrate NO4 does not
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Phenol.  If a proton attaches to the oxygen in Phenol, the positive charge can be stabilized in the aromatic ring by resonance.
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PH3:                           Phosphine\nAg2SO3:                    Silver Phosphite\nFeCO3:                      Iron(II) Carbonate\nN2O4:                        Dinitrogen tetroxide\nPb(OH)2:                   Lead(II) Hydroxide
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It is an electrophilic aromatic substitution reaction.  Because the -COO- acts as an electron withdrawing group to one phenyl group and a moderate electron donating group to the other pheny group the nitration will occur on the pheny group where the COO- is acting as an electron donating group.  The major product of the nitration will have the -NO2 in the para position because the ortho position is partially blocked by the large COPh group.\n\nI hope this helps!
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Phosphorus forms only oxy-hydroxides, like phosphoric acid (H3PO4), which could be written as PO(OH)3. There will always be one H2O less than theoretically possible.
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Hypophosphoric acid, H4P2O6, is a tetra basic acid, prepared from NaClO2 and red phosphorous. As to its structure, I don't know, but just try arranging all the atoms in that compound in such a way as to satisfy all their valencies.
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para-nitroacetophenone, in other words.\n\nMy first inclination is a Friedel-Craft acylation followed by a nitration with nitric acid in sulfuric acid (the nitronium ion). But the addition of the acetyl group would direct the nitro group to the meta position.\n\nMaybe if you nitrate the ring first and reduce the nitro group to an amino group. Then you could Friedel-craft to get the ketone at the para position (with some ortho isomerism). You'd have to find a way to oxidize the amino group to a nitro group ... I don't know how.\n\nAnother method would involve oxidizing toluene with KMn04, to get benzoic acid. You could then esterify the benzoic acid. Using DIBALH (Diisobutyllithium aluminium hydride), you could get an aldehyde (1-phenyl-methanal). You could use a Grignard reagent (methyl magnesium bromide) to get the alcohol with a methyl group added. You could then oxidize the alcohol with PCC to get a ketone. Finally, you could nitrate the ring with nitric acid and sulfuric acid.\n\nI'm not sure if either synthesis is perfect; My second one is long and rather expensive, in terms of reagents. Also, PCC is toxic (chromium) and many of the reducing agents are water sensitive.
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Greetings,\n\nNitrous Oxide.\n\nFor more informations follow the link.\n\nhttp://www.chm.bris.ac.uk/motm/n2o/n2oc.htm\n\n-matt
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what affects buffers?\n\ndepends on which bufffers  -pH will with solubility, aas will temperature\n\nmaximum capacity depends on individual buffer - citric acid maxes at 3 base molecules, as does phosphates..\n\n\nnow to the question - what will you do for me?????   Good  thing I am a Christian - so i'll just take a thank you