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Intramolecular definition +examples
Within the molecule (ionic, covalent)
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Intermolecular
Between the molecules (van der waals, dipole-dipole, hydrogen)
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value of R in PV=nRT
.0821 atm L/mol K
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Dalton's Laws of Partial Pressure
- PT=ΣPi
- PT=VP+Pi
- Pi=XiPT (X=mole fraction)
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Making a molar solution
- Obtain volumetric flask
- Rinse with soapy water
- Rinse with regular water
- Rinse 2-3 times with DI water
- Calculate g solute needed
- Fill flask 1/2 full with DI water
- Add correct g of solid using a funnel
- Cap/shake to dissolve
- Add DI water to within 1cm of marking
- Add drop by drop until mark is met
- Cap/shake
- Place in storage bottle
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PPM and PPB
1/106 and 1/109 units must be the same (g/g)
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Solubility of gas in liquid (related to temperature)
As temperature increases solubility decreases
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Solubility of gas in liquid (related to pressure)
As pressure increases solubility increases
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Colloidal dispersion
- Homogeneous
- Small enough to pass through filter
- Too large for semi-permeable membrane
- Can be seen with light
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Suspensions
- Heterogeneous
- Too big for filter
- Too big for semi-permeable membrane
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Colligative properties
Properties that depend on # of particles, not type of particle
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Isotonic values
- .3 M
- .9%m/v NaCl
- 5%m/v Glucose
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Shrinking and swelling
crenation and hemolysis
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Solution
- Homogeneous
- Can't be filtered
- Will go through semi-permeable membrane
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Standardized
Determine molarity to +/- .001M
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Proof of a reaction?
- Solid
- Weak electrolyte (heat)
- Gas
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Arrhenius acid/base
Produces H+/OH- in solution
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Bronstead-Lowry acid/base
H+ donator/H+ acceptor
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Conjugate acid/base formula
HA+B<--->A-+HB
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Examples of molecules that are both acids and bases
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H2SO4
Car batteries, Plant fertilizer
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HNO3
Explosives, Fireworks, Fertilizers
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HC2H3O2
Vinegar, food, plastics
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H2CO3
Carbonated beverages, blood
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NaOH
"Caustic lye," soap, drain cleaner
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NaHCO3
Antacid, baking soda
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NH3
Detergent, fertilizer, glass cleaner
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Litmus colors
acid - red, base - blue
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pH from [H+]
pH = -log[H+]
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pH and pOH relationship formula
pH + pOH = 14
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[H+] from pH
[H+] = 10-pH
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Larger Kameans...
stronger electrolyte (more dissociation)
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[H3O+] from [OH-]
[H3O+] = 1.0x10-14/[OH-]
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[OH-] from [H3O+]
[OH-]=1.0x10-14/[H3O+]
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Nitrite buffer system
HNO2 / NaNO2
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Acetate buffer
HC2H3O2 / NaC2H3O2
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How does a buffer system maintain pH?
- weak acid combines with strong base to create H2O and conj. base
- Conj. base combines with H+
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Buffer systems in body
- H2CO3 / HCO3-
- H3PO4 / H2PO4- / HPO42- / PO43-
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