Test 2

electrolyte strength

associated w degree of ionization of an electrolyte in aq sln, and number of ions (per mole) produced via ionization

equilibrium constant

K, only changes when temp of rxn changes, coefficients in rxn become the powers in the constant. it is a magnitude with no units

activity a

effective concentration or pressure, gamma is the activity coefficient equaling 1. this is true for all solids and liquids part of rxn

very small magnitude of K

almost entirely reactants, barely proceeds

intermediate

mix of reactants and products

very large magnitude of K

almost entirely products, goes to completion

Kow

octanol-water partition coefficient, when something is dissolved in octanol, measures the lipophilicity/ hydrophobicity of a solute. (large Kow, high lipophilicity)

three characteristics of Persistent Organic Pollutants

persistence (resists chemical/ biochemical transformation), toxicity (acute and/ or chronic), and bioaccumulation/ biomagnification (concentration in fatty tissues (high Kow), further amplification up the food chain)

Le Chateliers Principle

when equil system is subjected to stress, it responds by attaining new equil. stress can be temp, pressure, concentration change.

instances of la chateliers principle

decrease volume (increase pressure)→ less moles gas. increase volume (decrease pressure) → more moles of gas. raise temp→ direction of endothermic rxn. lower temp→ direction of exothermic rxn

Reaction quotient

Q. ratio of products to reactants at any instant. not a constant, is used to measure direction of rxn

Q to K comparison

Q>K, to the products. Q<K, to the reactants. Q=K, at equil

why is Fluoride in toothpaste

bc Fluoride can take the spot of OH when it is gone and is 460 times less soluble in Flurapatite than hydroxapatite.

Ion product

Qsp. predict whether precipitate will form.

Qsp to Ksp

Qsp>Ksp rxn shifts left, precipitation should occur, supersaturated. Qsp<Ksp, rxn shifts right, precipitation does not occur, unsaturated. Qsp=Ksp, no shifting, precipitation already occured, saturated

Arrhenius Theory

electrolyte dissolution behaviour, acids ionize to generate proton, bases ionize to produce hydroxide. applicable to protic acids and metal hydroxides in water, but has many exceptions (like NH3)

Bronsted-Lowry Theory

acid is a Hydrogen donor, base is a Hydrogen acceptor. with addition of water, CB is Acid minus an H, CA is Base plus H.

Lewis Theory

acid is electron pair acceptor, base is electron pair donor (e pair is shared). curved arrows to show e flow (- to +). least restrictive definition, can show aq or non-aq, unusual non-protic systems.

Acid equilibrium constant

Ka=[H3O+][A-]/ [HA], acid dissociation constant. >>1 means products dominate, <<1 means reactants dominate

base equilibrium constant

Kb=[OH-][BH+]/ [B], base dissociation constant. >>1 means products dominate, <<1 means reactants dominate

strong acids to know

HI, HCl, HBr, HClO4, HNO3, H2SO4(only 1st ionization is taken)

strong bases to know

Group 1&2 hydroxides, Group 1&2 hydrides (H-), and Group 1&2 Oxides

auto-ionization of water

water is amphoteric, undergoes acid-base rxn w itself, defines pH scale, PKw=pH+pOH=14.0. pH=-log[H3O+], [H3O+]=10^-pH (and same for OH just add OH to rxn and subtract from 14 if given pH)