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Will water with salt evaporate faster than water without salt?
Transcript of Will water with salt evaporate faster than water without salt?
http://van.physics.illinois.edu/qa/listing.php?id=1461 Bibliography My major results was figuring out which evaporated faster and how long did it took for both to start evaporating, the pure water evaporated faster than the water with salt, and it took the water without salt 1 hour to lower down to 1/4, but the water with salt took about 2 hours to lower down to 1/4. The result did supported my theory, because my theory was that the water without salt would evaporate faster than water without salt. My results turned out to be what my research was, every research I had found was the same the water without salt will evaporate faster. This happened because the salt keeps the water from evaporating due to the salt increasing the boiling point of the water, so the water needs more boiling point in order for the water to evaporate faster than the water. Conclusions The result turned out to be what my theory was. The water without salt evaporated faster than the water with salt. Using a warm temperature the water took about 1 hour to get to 1/4, but the water with salt took 2 hours to start evaporating and lower down to 1/4. I figured out that the surrounding of both cups were warm it took a lot of energy for the water with salt to start evaporating, but it didn't take much energy for the plain water to start evaporating. Results Step 1: Get 2 cups out the off cupboard
Step 2: fill both cups with the same amount of water. (2/3 of water you can use the measuring cup to measure the water)
Step 3: Get a spoon and then fill it with salt then deposit it in one cup.
Step 4: Turn the oven into a warm temperature. (120 Fahrenheit or 50 Celsius)
Step 5: Insert the 2 cups inside the oven,
Step 6: Wait, Then take notes every 5 minutes. Procedure 2 Cups oven safe
2 Teaspoons of table salt
Measuring cup Materials If you put salt in the water it takes a lot of energy to take out the solute out of the water and turning it in to air, and happening so it can make the salt dissolve very easily. The water will boil if the vapor pressure reaches the pressure of the atmosphere, in order to do this you need to heat the water with solutes more to get the vapor pressure to equal the atmosphere. Source 2 –Mike. Tom. Q&A: Salt and the boiling point of water Department of Physics University of Illinois at Urbana-Champaign
October 22 2007. December 7 2012
http://van.physics.illinois.edu/qa/listing.php?id=1447 Background Research If salt in a water and pure water is to be compared to see which one evaporates faster, my hypothesis would be that water without salt would evaporate faster than water with salt. Hypothesis The following experiment we are trying to figure out which evaporates faster. Water with salt or without salt? This information can be useful to the scientist knowing how much water will evaporate from a water body with a specific amount of salt, and how much energy it will take in order to evaporate. Calculating the energy cost to vaporize a certain amount of water at a different amount of contained salt. Purpose By: Clarence Garcia
I chose this topic because, I was curious which will evaporate faster, and how much time it would take for both to evaporate. Will water with salt evaporate faster than water without salt? Data Analysis The salt makes it difficult for the water to evaporate, because the salt increase the boiling point of the water and it takes a lot of energy for the water to start evaporating. The water needs to start boiling in order to evaporate faster, the salt breaks away from each other then forms a ions which is negative and positively charged. Source 5 – Hess, Amber. Salt Water Evaporation Science Fair Project.
Science Buddies. April 12 2010. December 7 2012
http://www.sciencebuddies.org/science-fairprojects/phpBB3/viewtopic.php?f=36&t=6314 Background Research
This article tells us that the freezing point of a water is 32 degrees Fahrenheit and the water boils at 212 degrees Fahrenheit. The reason why the salt water to evaporate because its boiling point raised and the water needs to be 212 degrees to continue evaporating faster than a regular water. Also the pure water has more freezing point than boiling, and it evaporates faster if its colder, but since the salt was added to the water the waters boiling point raises. Source 4 – Unknown. Effect of Salt on the Boiling Temperature of Water.
Action Donation Services. January 11 2013
http://www.actiondonation.org/articles/effect-of-salt.html Background Research Source 3 –
Calder, Vince .Gregorius, Roberto. Zimmerman, Burr. Salt, Fresh Water Evaporation Experiment
Newton Ask A Scientist!. June 2007. December 7 2012.
http://www.newton.dep.anl.gov/askasci/gen06/gen06351.htm This article tells us that the salt makes it hard for the water molecules to evaporate, so the water without salt evaporates more than water with salt. The pieces of water ten to stick around the salt molecules, while the water is evaporating the salt will stay, and the concentration of the salt also goes up while it evaporates. The speed of the evaporation can be controlled on how much salt you deposit in the water. So the longer the water stays the slower it evaporates. Background Research Salt increase the boiling point of a water and decrease the freezing point of the water. So if you put a pure water and water with salt in the freezer the pure water would freeze first because the freezing point of it is much higher than the boiling point, on the other hand the salt water would still be liquid. This just shows that the salt affects the water, the same with evaporating. Water usually evaporates at all temperatures about freezing level, but salt brings heat in the water which makes it difficult for the water to start evaporating. So when the salt water is put on a stove it starts boiling first than water with salt, because of the heat the salt has given the water. Source 1 – Mike. Tom. Q&A: Evaporating Saltwater. Department of Physics University of Illinois at Urbana-Champaign
October 22 2007. December 7 2012
http://van.physics.illinois.edu/qa/listing.php?id=1461 Background Research