Molality and Colligative Properties
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- เผยแพร่เมื่อ 10 ธ.ค. 2015
- Solute particles interfere with the physical processes a solution may undergo. These are known as the colligative processes of a solution. Ever wonder why we put salt on icy streets? Find out here!
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Vapor Pressure and Freezing Point Depression would be some pretty ａｅｓｔｈｅｔｉｃ names for a band, not gonna lie.
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This is one of colligative properties,isn't it ?
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Thank you for finally explaining Depression in freezing point to me after countless teachers have failed. It finally makes sense now.
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the particles with greater atomic or molecular size occupy more surface and cause a greater lowering in VP but you say it depends only and only on the number of solutes particles?
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Do you have a Kb and Kf reference to share, please? I currently cannot find one.
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When he said Let's test comprehension it almost hurt my little pea sized brain.
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dont you have to account for the particles in the compounds?
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hey! so I totally understand freezing point depression from the perspective of solutes messing with the crystal lattice structure of solids. but I'm currently studying for the mcat and i was reading online that, above the freezing point, the vapor pressure of a liquid is greater than that of the corresponding solid, and that the opposite is true below the freezing point. and that the vapor pressures of the two phases are equal AT the freezing point. so if we think about it in these terms, if we add solute to a liquid, thereby lowering its vapor pressure, wouldn't that actually raise the freezing point (i.e. make it more "easily freezable")? because wouldnt the vapor pressure of the liquid now be closer to that of the solid? I know this obviously doesnt happen in nature because salt trucks would be causing more problems and not less. but just trying to understand freezing point from the perspective of vapor pressures. thanks!
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Nice video, very helpful. Also osmosis is affected from solute concentration.
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Why isn't the van 't Hoff factor used in this video?
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Why isn't van't Hoff's factor (i) in those colligative formulas'?
can you please make soem content on equivalent weight
Dear Dave,Can u make a video on vapour pressure seperately , i wanna know more about how its calculated and the related facts
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Is there any way to somehow elevate freezing point and depress boiling point?
I always thought that salt accelerates boiling of water due to it having lesser heat capacity (heard that somewhere).
This video made me think and...
1) The supposed change in heat capacity from adding 1 mole of salt to 1 liter of water (55.5 moles) is ~0.5%, with same negliglible heating speedup
2) You'd have to spend extra 1/56 energy on heating salt itself too, so 1.7% slowdown.
3) The boiling point of solution is raised by 0.51 degrees, so another ~1% slowdown assuming water is at 25 degrees initially.
So salty will actually boil slower than "pure" water - the tap water already has some dissolved compounds, though.
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The definition of colligative properties saved my life
what happened to the freezing of water when salt is added?
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