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Lec 25 | MIT 3.091 Introduction to Solid State Chemistry

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Uploaded by on Apr 29, 2008

Solutions: Solute, Solvent, Solution, Solubility Rules, Solubility Product

View the complete course at: http://ocw.mit.edu/3-091F04

License: Creative Commons BY-NC-SA
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  • GOD OF ALL CHEMISTRY PROFESSORS

  • thanx soo much for these. he's really great. helped me a lot!!!!!!!

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  • fuck

  • love you man

  • Lol >> We have smart boards :)-

  • Now, that is teaching!!! Awesome!!

  • @1091Floyd21 no they do not combine, they fully dissociate (break down into individual ions) Think of it like this: the Ag, NO3, Na and Cl ions all break down into individual ions. They are free-floating particles flying around the solution, all individually. If they are insoluble, (Ag and Cl) they stick together, forming a larger molecule, which then settles to the bottom (precipitate). If they are soluble, then they do not stick, so they continue to float around individually (Na and NO3)

  • @tallguy111 But do they combine with each other or what? the Na+ & NO3-?

    Cheers

  • @1091Floyd21 they are spectator ions, and can be removed from the equation, leaving you with the following : Ag+(aq) + Cl-(aq) --> AgCl(s)

  • In the following reaction to test for the presence of Cl ions: AgNO3 + NaCl => AgCl + ( ), what goes in the space. I mean what happens to the NO3- & the Na+ ????

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