ch5a - Chemistry 1110/1210 Dr Eric E Moore Section 5.1...

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Chemistry 1110/1210 Dr Eric E. Moore Section 5.1 Section 5.2 Section 5.3 Section 5.4 Section 5.5 Section 5.6 Section 5.7 Section 5.8 Section 5.9 Section 5.10 Section 5.11 Section 5.12 Section 5.13 Chemistry 1110/1210 Chapter 5 Dr Eric E. Moore St John’s University September 26, 2007
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Chemistry 1110/1210 Dr Eric E. Moore Section 5.1 Section 5.2 Section 5.3 Section 5.4 Section 5.5 Section 5.6 Section 5.7 Section 5.8 Section 5.9 Section 5.10 Section 5.11 Section 5.12 Section 5.13 1 Section 5.1 2 Section 5.2 3 Section 5.3 4 Section 5.4 5 Section 5.5 6 Section 5.6 7 Section 5.7 8 Section 5.8 9 Section 5.9 10 Section 5.10 11 Section 5.11 12 Section 5.12 13 Section 5.13
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Chemistry 1110/1210 Dr Eric E. Moore Section 5.1 Section 5.2 Section 5.3 Section 5.4 Section 5.5 Section 5.6 Section 5.7 Section 5.8 Section 5.9 Section 5.10 Section 5.11 Section 5.12 Section 5.13 Solutions A “Solution” is a homogeneous mixture in which one substance (the “solute” is uniformly distributed throughout a second substance (the “solvent” ). The amount of solute dissolved in the solvent is it’s “concentration” .
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Chemistry 1110/1210 Dr Eric E. Moore Section 5.1 Section 5.2 Section 5.3 Section 5.4 Section 5.5 Section 5.6 Section 5.7 Section 5.8 Section 5.9 Section 5.10 Section 5.11 Section 5.12 Section 5.13 Concentration Concentration can be measured several ways, one is in terms of “percent concentration” , which is just the mass of the solute divided by the mass of the solute plus the mass of the solvent. A solution with a lot of solute in it is described as being “concentrated” and a solution with relatively little as being “dilute” .
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Chemistry 1110/1210 Dr Eric E. Moore Section 5.1 Section 5.2 Section 5.3 Section 5.4 Section 5.5 Section 5.6 Section 5.7 Section 5.8 Section 5.9 Section 5.10 Section 5.11 Section 5.12 Section 5.13 Saturation If you keep adding solute to your solution, and it doesn’t dissolve (it remains solid and sinks to the bottom making a heterogeneous mixture), then the solution is described as “saturated” . If less solute is in solution than can be dissolved, a solution is “unsaturated” .
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Chemistry 1110/1210 Dr Eric E. Moore Section 5.1 Section 5.2 Section 5.3 Section 5.4 Section 5.5 Section 5.6 Section 5.7 Section 5.8 Section 5.9 Section 5.10 Section 5.11 Section 5.12 Section 5.13 Precipitation A solution that has more solute in it than a saturated solution is “supersaturated” . Solutions tend not to remain supersaturated long, and the excess solute separates into a different phase. When this different phase is a solid forming from a liquid solution, we describe the solid as a “precipitate” , and the process of the solid forming as “precipitation” .
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Chemistry 1110/1210 Dr Eric E. Moore Section 5.1 Section 5.2 Section 5.3 Section 5.4 Section 5.5 Section 5.6 Section 5.7 Section 5.8 Section 5.9 Section 5.10 Section 5.11 Section 5.12 Section 5.13 Ionic solutions When ionic compounds are added to water, they sometimes dissolve. When they do so, they “disassociate” into their separate ions.
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