LAB PRACTICAL Flashcards by Callie Hill

Measurement estimates

one value beyond the last marking on measurement device

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Pharmacokinetics

process by which drug is absorbed, metabolized, eliminated

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Catalysis

increase in rate of reaction due to participation of catalyst which lowers activation energy

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Order of reaction

determined by coefficient in balanced equation but must be determine EXPERIMENTALLY

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Arrhenius Equation

k = Ae^_Ea/RT with R = 0.008314, Ea = activation energy

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Greater activation energy means

slower rate

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Chemical Kinetics Reaction Rate

Rate = k [Fe3+]m[I-]n (we determined m and n experimentally)

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Chemical Kinetics Rate in terms of Triiodide ion

Rate =Δ[I3-] / Δt

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What was Fe3+ conmibed with

I- and S2O3 2-

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Chemical Kinetics Plot

y = ln(Rate) x = ln([I-]_ with slope = n

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Methyl green

green color with seven methyl groups attached, parent dye has 0 groups

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Rate of Decolorization [OH-]

[OH-] = 4.5 x 10^-2 x [PO4 3-] / [HPO4 2-]

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Rate of Decolorization rate law

rate = k1[dye][H2O] + k2[dye][OH-]

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Dye and Absorbance

[dye] = A / e L
-lnA = kobst -lnA0

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Graph -lnA versus time

slope is observed rate constant

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What is the slope of Kobs vs. [OH-] equal to

= K2, kobs = k1[H2O] + K2[OH-]
K1[H2O] remains constant and does not effect slope (acts as an intercept)

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ΔG°= (2 equations)

ΔG° = ΔH° - TΔS°
ΔG° = -RTlnK

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If K > 1

ΔG° < 0 and the process will proceed in the forward direction

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lnK =

lnK = -ΔH° / RT + ΔS° / R

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Ksp is independent or dependent on temperature

dependent

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Plot lnK versus 1/T

slope is -ΔH°/R

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Ice cream freezes

at a lower temperature than the freezing point of water so rock salt is added

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m =

m = moles solute / kg solvent

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is molality temperature dependent or independent

independent

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Vant Hoff Factor

number of dissolved particles the solute contributes

m = (with VHF)

m = Δtf / I kf

Natural dye in solar cell experiment

TiO2 stained and dye absorbs light from sun to produce flow of electrons

Semi conducting material

TiO2, titanium dioxide

How to electrons flow in solar cell

from TiO2 coated electrode to the counter electrode producing electricity

What does the dye molecule release when it absorbs light

electrons

Mediator

Iodide ion in the electrolyte

Voltage

difference in energy levels of TiO2 and mediator

Current is directly proportional to

amount of light or number of photons absorbed by the dye

Power of solar cell

voltage x current in Watts

Compound in raspberries that plays a role in solar cell

Anthocyanin (carbohydrate) (REVIEW STRUCTURE)

Chelation

bonding in ions and molecules to metal ions, involves presence of two separate bonds between polydentate ligand and single central metal atom (REVIEW STRUCTURE)

Mediator oxidation

I- + I2 <--> I3 -

Mediator reduction

6e- + 3I2 <--> 2I3-

Common uses of TiO2

toothpaste and food coloring

Area of solar cell to produce 1 watt?

1 watt = Power Watt x Area

Commercial vinegar contains

5-6% acetic acid

Percent Error =

Absolute Value of Actual - Experimental / Actual x 100

Molarity Calculations

M1V1 = M2V2

Percentage (w/v) acetic acid in vinegar

mol / L x 1L / 1000 mL x 5.00 mL = mol x mol x g / mol = x g / 5.00 mL = X x 100

Examples of coordination compounds

hemoglobin, vitamin b12, chlorophyll

Ammonia serves as

ligand

Sulfate ion serves as

counter ion

Copper coordination compound formula

Cux(NH3)y(SO4)z x H2O

Color indicator in volumetric analysis of ammonia

methyl orange

Beer Lambert Law

absorption of light as it passes through solution is proportional to the concentration of the absorbing species

Empirical formula

Cu(NH3)4(SO4)

Bonsted-Lowry acid

proton donor

Strong acid

ionizes essentially to completion

Larger Ka

stronger acid

Equivalence point

final solution neutral (equal moles), where amount of base has been added, + 1 drop is light pink, vertical on curve

End point

1 final drop turned light pink

After reaching equivalence point

pH is high due to excess base

Ka =

Ka = [A-][H3O+] / [HA]

Ionization equation

[A-] = [H3O+] because 1:1 mole ratio

Titration data M

MaVa=MbVb Ma=MbVb / Va

Percent ionization =

% = [H3O+] / Ma x 100

Buffer solution

contains weak acid and conjugate base

Henderson-Hasselbalch

pH = pKa + log [A-] / [HA]

Halfway point

pH 1/2 = pKa

1st derivative

max, equivalence point, intersection with x-axis

2nd derivative

inflection point, change = 0

Saturated solution

in state of dynamic equilibrium between dissolved, dissociated, ionic compound and undissolved solid

The solubility of an ionic compound is

lower than a solution containing a common ion than in pure water

Ksp Barium Nitrate

Ksp = [Ba2+][NO3]2

Dynamic Equilibrium

rate of forward = rate of reverse

Equilibrium constant

Keq = [products] / [reactants]

Equilibrium constant graph

y axis = A/([Fe3+]I [SCN-]I) x axis = A x ([Fe3+]I + [SCN-]I) / ([Fe3+]I [SCN-]I) slope = -Keq

Freezing point

temperature when solvent in solution and pure solid have same vapor pressure

Larger Ka

more ionization and stronger