what is the boiling temperature disstalled water?
814502
at 1atm it's 212 F or 100C.  That's only at 1atm.
131793
Various minerals that exist in the water could cause the boiling point to fluctuate.\n\nAs an example, people add salt to water that they are boiling in order to lower the boiling point of the water.  On the converse scale, salt is also used to lower the freezing point as well, which is why roads are salted to avoid icing of the surface.\n\nAside from sodium, water can contain other natural minerals, which will also affect the boiling and freezing points.  Elevation and pressure will also have an effect on this as well, depending upon whether you are at or below sea level.\n\nI imagine that if you were perfectly at sea level, boiling only distilled water, it would probably be the closest to 100 degrees that you can get.
141221
The original water temp is 25C, as was given in the problem... I'm assuming you meant to ask what was the initial temp of the water that was added, which isn't too hard. Here goes.\nQ(heat)= m(mass) x c(specific heat) x delta T(change in temp)\nso Q = (150g)(4.something J/gC-look it up)(25C-14C)\nBecause of conservation of energy and assuming ideal insulation, the heat LOST by the 150g of water during the mixing is equal to the heat GAINED by the 200g of water. So, once you have Q, rearrange the equation to look like [delta T] = Q/mc = Q/(200g)(c)\nThat will give you the temperature difference between 14C and the 200g of water's initial temp. Delta T should come out as being positive, since the temp is going up. \nWhen you have more complex mixtures of things with different specific heats and add processes and changes, the math becomes a lot more of a headache but the same basic principles apply just the same.
748490
If you are asking how to separate a mixture of water and salt, then you need to distill the water.  Distillation separates materials by adding increasing amounts heat in order to boil off the materials at theri respective boiling points.  The material that boil at a lower temperature would be removed first.  As you increase the tempreature, higher boiling temperature materials are separated.\n\nSince the water boils and the salt does not, all you need to do is heat the mixture up until it boils.  The water will vaporize and can be captured in another container, leaving the salt behind in the original container.
39906
Liquid nitrgen absorbs heat as it boils away. Its boiling temperature at normal atmospheric pressure is about -270 deg F. Almost all mechanical refrigeration uses a boiling substance (refrigerant) to absorb heat. \n\nREK Mechanical engineer
341668
Water evaporates at 100 degrees, celsius, so the liquid water you touched wouldn't be any hotter than that. The metal, on the other hand, does not. So it would be as hot as the object which is heating it.
581795
The highest temperature water in liquid form can reach is the boiling point.  At this point the water will change from a liquid phase to a gas.  For pure water, this initial temperature is 100 deg Celcius.  For salt water, the  water will reach about 100.5 deg before turning into a gas.  Once it becomes a gas it usually escapes direct contact from the heat source and cools and condenses back into a liquid form that is suspended in the air in the form of tiny droplets (this is the steam that you see).  Since any salt will remain behind as the liquid boils into a gas, the gaseous water from both sources will condense back into the steam that you see at 100 degrees.  So I guess you could say that the initial temperature of boiling water from salt water is slightly higher but once it becomes the white misty steam that you see, the two are basically the same temperature.
562654
Okay, I'll try this one -\n\nRun this experiment twice (or more times), each time with a piece of metal having different density.  The metal piece should be of adequate size (a sewing needle isn't going to do it), it needs to be big enough to significantly affect the temperature of the water.  You will need to know the mass of the metal (i.e., weigh it) and have a thermometer capable of reading from room temperature up through boiling or so.  Please note this is not going to give you a highly accurate answer, but can give you a ballpark idea (I'm guessing you're probably not doing this in a 500 million dollar lab).\n\nThe procedure:\n\n1)  Measure and record room temperature as T1.\n\n2)  Weigh the metal, call it M1.\n\n3)  Bring a known quantity of water (weigh it, or measure it and convert to weight, call it M2) to a temperature just short of boiling (say 180F to 200F, use the same temperature for each run of this experiment).  Record the temperature as T2, and remove the heat source (take it off the burner, etc.).\n\n4)  Drop in a metal piece at room temperature.  Allow a couple of minutes for heat to exchange.  Make sure you use \nthe same amount of time for each run of this experiment.\n\n5)  Measure and record the new temperature of the water as T3.\n\n6)  Repeat with your other metal samples.\n\nYou can now estimate the specific heat capacity for each metal.  It will not be super-accurate (heat escapes your system, and temperatures won't have completely equalized), but should give you some idea.  Just assume all temperatures did equalize and that no heat escaped for calculational purposes.\n\nSince (you are assuming) the heat which left the water went into the metal, then the product of mass, specific heat capacity, and temperature change should be the same for both the metal and the water (but in opposite directions).\n\nThis means that:\n\n(M1)(c1)(T3-T1) = (M2)(cw)(T2-T3)\n\nwhere c1 is the specific heat capacity of the metal, and cw is the specific heat capacity of water (look it up on Google to get the units you need).\n\nSolving this, you get:\n\n......(M2)(cw)(T2-T3)\nc1 = -----------------\n........(M1)(T3-T1)\n\n(sorry about the dots, I'm trying to keep everything aligned)\n\nRepeat the calculations for each of the metals.\n\nYou will need to calculate (or look up) the densities of each of the metals.  Then, graph density vs. the specific heat capacities you calculated, and see if your hypothesis is true.\n\nHave fun!
872856
It will eventually melt at 2572C, and it will boil at 2850C.\n\nHeat does not cause it to react, typically.
195177
It  isn't boiling.\n\nIt steams because it is well above the temperature of the surrounding air.\n\nWhen the air heated by the hot water in the teacup rises, and reaches the cooler room of the air, the moisture condenses.\n\nBoiling is 212 F. Room temperature might be 70 F.
849983
low pressure = lower boiling point = lower dew point
297542
well lets see, if cold water is anything above 0 Centigrade and hot water is anything under boiling....my money is on the hot winning. What I can not understand is why you asked?
745608
liquid...at 0 C it would be frozen and at 100 C it would be gas, since 75 is not yet boiling, the water would still be liquid
505556
you have to look for it at the saturated watter boards or the saturated water graph, then the temperature will tbe the saturation temperature, according to my graph, the temperature would be...\n\n83.79ºC
875611
Boiling and non-optimal pH denature enzymes.
585025
I don't know that you can, different solvents react differently to pressure, so I don't think it's a one eqaution fits all kind of process.  That's why they all have different graphs for phase vs temperature/pressure.  I'm sorry.\nSounds like you have a pretty high boiling point though, the things I've taken off that had to be real high temp were water, toluene, and pyridine.  Could it be one of them?  They smell pretty different, so you'd know which.  \nThat's an interesting question though, I've never stripped a solvent that I didn't know what it was.
209192
Boiling Point: \n204C (399F) \nMelting Point: \n100C (212F) \n\nCHECK IT OUT BUT I THINK ITS CORRECT