Acids and Base Equilibrium
Acids and BasesTypes of Acids and Bases Arhennius- based on ions Bronsted- Lowry- based on Protons Lewis- based on electrons Formulas
ph=-log [H+] (where H+ is concentration) 10^(-ph)= [H+] (where H+ is concentration) pOH=-log [OH] where OH is concentration 10^(-pOH)=[OH]where OH is concentration Naming Acids and Bases-ide-ite-ate |
EquilibriumMaking ICE Tables- http://www.chem.purdue.edu/gchelp/howtosolveit/Equilibrium/ICEchart.htm#HowtomakeICE Le Chatelier's PrincipleWhen a reaction is stressed the reaction shifts to the direction of less stress to reach equilibrium.
Temperature StressIn an Endothermic reaction temperature and product are directly related when stressed. In other words an increase in temperature will give us an increase in product and a decrease in temperature will give us a decrease in product.
For Exothermic reactions the relationship between temperature and the shift of a reaction is inverse. In other words increased temperature means more energy in a system and no need for energy to be released as a product and less temperature means there is a need for more energy in the system and increases the release of energy from the exothermic reaction. Pressure StressPressure is produced by a change in volume. By increasing the pressure the shift is place toward the product because molecules are closer together and more likely to interact. As you increase volume you increase space and decrease pressure causing less interaction and reaction and less product to be produced.
Concentration StressIncreasing the concentration, specifically that of the limiting reactant will increase the product that is produced. Adding product to a reaction will also shift the reaction the opposite direction towards reactants. The removal of product increases product by decreasing reactants and the removal of reactants decreases product.
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