Net ionic equations & KSP (lecture 1)

UNIT 2

solution

a homogenous mixture containting 2 or more substances

solvent

component that determins the phase of the solution

solubility

maximum amount of a solute that can be dissolved in a given solvent at a given temperature

saturated solution

max amount of solute has been dissolved

unsatured solution

more solute can be dissolved

supersaturated

has more dissolved solute than can be dissolved under normal conditions

strong electrolte

a substance that completely or almost completely dissociates into ions when dissolved in water (high electrical conuctivity)

exampales of strong electrolytes

strong acids and bases, salts

weak electrolytes

ionize partilally in water (low eelectrical conductivity

examples of weak electrolytes

weak acids and bases

non electrolyte

mplecular compund that dissolves in water (no electrical conducitiy)

examples of non electrolytes

sugars and alchohols

precipitate

insoluble solid

ksp (Solubility Product Constant)

indicates the maximum amount of an ionic solid that can dissolve in a solution, with a larger Ksp value signifying greater solubility.

ksp and staturated solution

ksp = IP (ion product

ksp and unstaturated solution

Ksp > IP (ion product)

ksp and superstaturated solution

ksp < IP (ion product)

molar solubilitity

actual amount (concetration) of solute that can exist in an satruated solution at eqauilibri

how does having a ion present in a solution affect its ability to dissolve

its cannot dissolve as much of that ion

steps to solve for molar solubity

1. idenfity common ion and insoluable salt

2. write ksp expression for insoluable salt

3. plug in cocnentration of the common ion directly

4. solve for the consentration of the other ion. this is the new molar solubaility

which anion preceiitates first

the one with the smallest number aka smallest cut off