Unit 4 Part 2 Solutions. Components of a Solution A solution is composed of two or more pure...
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Transcript of Unit 4 Part 2 Solutions. Components of a Solution A solution is composed of two or more pure...
![Page 1: Unit 4 Part 2 Solutions. Components of a Solution A solution is composed of two or more pure substances, one of which is a solvent and the other a solute.](https://reader035.fdocuments.in/reader035/viewer/2022071807/56649e545503460f94b4ac1c/html5/thumbnails/1.jpg)
Unit 4 Part 2Solutions
![Page 2: Unit 4 Part 2 Solutions. Components of a Solution A solution is composed of two or more pure substances, one of which is a solvent and the other a solute.](https://reader035.fdocuments.in/reader035/viewer/2022071807/56649e545503460f94b4ac1c/html5/thumbnails/2.jpg)
Components of a Solution
A solution is composed of two or more pure substances, one of which is a solvent and the other a solute.
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Components of a SolutionA cup of instant coffee is the
____________, the hot water is the ____________, and the instant coffee is the ____________.
Solvent Solution Solute
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Components of a Solution Solutions in which water is the solvent
are called aqueous solutions.
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Water as a SolventMost covalent liquids are only
able to dissolve other covalent compounds; water can dissolve both ionic and covalent compounds.
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Water as a solvent
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Water as a solventThe attraction of water
dipoles for ions pulls ions out of a crystalline lattice and into aqueous solution.
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Solutions: A saturated solution is a solution that
contains the maximum amount of solute dissolved in a solvent. A supersaturated solution is a solution where conditions have been changed to allow more solute to dissolve than would at room temperature (this is done by heating the solvent or solution).
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Solutions: When the solvent and solutes are liquids
we can use the terms miscible and immiscible. Miscible means that the two liquids will mix together, and immiscible means that the two liquids will not dissolve in one another.
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Solutions: Sometimes when we mix two dissolved
salts together, we end up with a precipitate. This is because a new ionic compound is formed that is insoluble in water.
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Solutions: We can use solubility charts or solubility tables
to determine if a solid will be formed.Ion Solubility ExceptionsNO3
– soluble none
ClO4– soluble none
Cl– soluble except Ag+, Hg22+,
*Pb2+
I– soluble except Ag+, Hg22+,
*Pb2+
SO42- soluble except Ca2+, Ba2+, Sr2+,
Hg2+, Pb2+, Ag+ CO3
2- insoluble except Group IA and NH4
+
PO43- insoluble except Group IA and
NH4+
OH– insoluble except Group IA, *Ca2+, Ba2+, Sr2+
S2- insoluble except Group IA, IIA and NH4
+
Na+ soluble noneK+ soluble noneNH4
+ soluble none
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Solutions Ex. If we mix sodium ions with
hydroxide ions will a precipitate form?
Ex. If we dissolved sodium hydroxide in calcium chloride, will a precipitate form?
2NaOH + CaCl2 2NaCl + Ca(OH)2
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Solutions Ex. Calcium nitrate with sodium
carbonate Ca(NO3)2 + Na2CO3 CaCO3 + 2NaNO3
Ex. Silver Perchlorate and Calcium Iodide
Ca(ClO4)2 (________) and AgI (__________)
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DemonstrationsIon Solubility Exceptions
NO3– soluble none
ClO4– soluble none
Cl– soluble except Ag+, Hg22+, *Pb2+
I– soluble except Ag+, Hg22+, *Pb2+
SO42- soluble except Ca2+, Ba2+, Sr2+,
Hg2+, Pb2+, Ag+
CO32- insoluble except Group IA and
NH4+
PO43- insoluble except Group IA and
NH4+
OH– insoluble except Group IA, *Ca2+, Ba2+, Sr2+
S2- insoluble except Group IA, IIA and NH4
+
Na+ soluble noneK+ soluble none
NH4+ soluble none