rank the following in order of increasing boiling point:?
821954
Here you can find a list of elements and their boiling points!
2595
boiling point of water\nfreezing point of water\naverage temperature of the human body\naverage room temperature\nboiling point of their parents :)
209192
Boiling Point: \n204C (399F) \nMelting Point: \n100C (212F) \n\nCHECK IT OUT BUT I THINK ITS CORRECT
639322
Highest boiling point is Na3PO4 because of the most no. of ions in solution.(also has lowest freezing point)\nHighest freezing point is Sucrose because of the least no. of particles in solution.(also has lowest boiling point)
733447
Br+H20--->HBr+O\n\nNi(II)O+H20--->Ni+H202\n\nKO2+H2O--->KOH + H2\n\nHope that helps.
1118024
Acidic \n\nbelow 6 acidic above 7 basic
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I would say CH2O2 (I'm assuming you mean formic acid, not dioxirane), CH3CO2H, and water.  \n\n"Important" is a tough word here, as all of these compounds can participate in h-bonding to varying degreees, with water being the strongest and CH2F2 being the weakest.  That said, strong hydrogen bonding gives rise to many of the nifty properties of water and in all three cases the h-bonding is powerful enough to raise the boiling points to be significantly higher than what you would expect based on molecular weight.
15822
It mainly depends on the pressure (if we are talking about pure water). The higher the pressure, the higher the boiling point - it can be much lower (ex. high in the mountains) or much higher than 100 degrees C (the boiling point under normal atmospheric pressure). If we don't talk about pure water, then adding other chemicals (for example, table salt - sodium chloride) can raise the boiling point as well.
750030
1. Iron (III) Hydroxide\n2. Ammonium Iodide\n3. Aluminum Hydroxide\n4. Sodium Carbonate\nThis site also has many others and is a great place to confirm your answers!\nhttp://www.quia.com/jg/125193list.html\nGood luck!
879801
Pentane\n\nIt depends on which compound has the strongest intermolecular forces. In the case of hydrocarbons the intermolecular forces that are present are dispersion forces.\nIn such cases:\n"The more branched a molecule is, the more "spherical" it is, and the smaller surface area it will have - since dispersion forces increase with surface area, the more branched molecules will have a lower boiling point. You may notice that the trend in the melting points is rather different - this is because the longer a branch is, the more potential it has to flop around and disrupt the regular crystalline lattice of frozen pentane, giving a liquid state."
777060
Tap water. Dissolved salt raises the boiling point, so salt water  takes longer to boil.
17774
It doesn't give me room to list them all and explain them on here so let me direct you to a website I found that does a pretty good job:\nhttp://vergil.chemistry.gatech.edu/notes/quantrev/node20.html
80429
The CRC Handbook of Chemistry and Physics has all kinds of good information like that (although it is pricey).\n\nOr, search the web for the specific liquid of interest.
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HBr ---> H(+) + Br(-)\nH2SO3 ---> H(+) + HSO3(-)\nCH3-COOH ---> H(+) + CH3-COO(-)
524682
In order of decreasing concentration:\n\nNitrogen, oxygen, argon, water, and carbon dioxide
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The boiling point depends on the intermolecular forces.\nThe stronger the intremolecular forces, the more energy you need to break them and thus the higher the boiling point will be.\n\nPolar molecules attract each other through dipole-dipole forces. The higher the polarity, the more strong these forces will be (because you will have stronger dipoles)\nNon-polar molecules attract each other through dispersion forces which are much weaker than the dipole-dipole forces.\n\nTherefore polar molecules will have higher boiling points and as polarity increases the boiling point also increases.
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Sodium carbonate\n\nBarium difluoride\n\nCopper(II) nitrate\n\nNickel (II) sulfate