1 Solutions One substance dissolved in another substance.
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Transcript of 1 Solutions One substance dissolved in another substance.
1
Solutions
One substance dissolved in another substance
TEKS
10 (A) describe the unique role of water in chemical and biological systems;
10 (B) develop and use general rules regarding solubility through investigations with aqueous solutions;
10 (C) calculate the concentration of solutions in units of molarity; 10 (D) use molarity to calculate the dilutions of solutions; 10 (E) distinguish between types of solutions such as electrolytes
and nonelectrolytes and unsaturated, saturated, and supersaturated solutions;
10 (F) investigate factors that influence solubilities and rates of dissolution such as temperature, agitation, and surface area;
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Solution is...A Homogenous...
Mixture of two or more substances
(evenly mixed)
NaClNaCl HH22OO
It is a physical change …NOTNOT a chemical change
+ Salt WaterSalt Water
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No…Air is a solutionAir is a solution
Sterling silver is a solutionSterling silver is a solution
It can be gas
It can be solid
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Types of Liquid Solutions
Aqueous A solution with water as
the solventTincture A solution with alcohol as
the solvent.
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Insoluble When a substance cannot be dissolved in a solvent...
Oil Water
++ ==
Therefore, oil is INSOLUBLE in water.
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Limits of Solubility
SupersaturatedSupersaturated …more solute than the solvent can handle.
SaturatedSaturated … the point that no more solute can be added to the solvent or it will be ---
UnsaturatedUnsaturated … more solute can be added to the solvent
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Solubility GraphsSolubility of KCL
0
10
20
30
40
50
60
0 20 40 60 100
Supersaturated
Unsaturated
saturatedsaturated
Hold all that it can possible hold (at a given
temperature) - concentrated
Contain less solute than it can hold (at a given temperature) - Diluted
More solute then it can hold (at a given temperature)
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Ionization The formation of ions by
the action of a solvent in solution.
NaCl (salt) in to Na+ + Cl-
in waterIons are formed (+ or -)
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Dissociation Is the process of separating ions
during the formation of a solution … the more it dissociates, the stronger it is...
Na+
OH-
Na+
OH-
Na+
OH- Na+
OH-
Strong BaseStrong Base
OH-
NH4+
Weak BaseWeak Base
NaOH Na+ + OH-
OH-
NH4+
NH3NH3
H2O
H2
O
NH3 + H2O NH4+ +
OH-
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Solution Concentration Refers to the amount of solute
dissolved in a solvent. Diluted (less)Concentrated (more)
5 grams5 grams of salt in of salt in 100 grams of Water100 grams of WaterDiluteDilute
VS.VS.
35 grams35 grams of salt in of salt in 100 grams of 100 grams of waterwater
ConcentratedConcentrated
100 g.
100 g.
5 g
35 g
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Electrolytes Because dissolved salts
have positive and negative ions, they are electrolyte solutions, and conduct electricity
NaNa++ClCl--
NaNa++
ClCl--
NaNa++
ClCl--
NaNa++ClCl--
NaNa++
ClCl--
ClCl--NaNa++