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chem

QuestionAnswer
Arrhenius acid compound that ionizes in water to form hydronium ions
bronsted acid proton donor
conjugate acid species that remains after bronsted base accepts H
Amphiprotic species that can donate and accept protons
Acid ionization constant (Ka) equilibrium constant of ionization of weak acid (HA) in water
Ka values Large Ka and small pKa means strong acid
Equilibrium constant(K) ratio of conc of products (raised to their coefficient) divided by reactants (raised to their co-eff)
K values Large K favors products(10^3), small favors reactants(10^-3)
When to neglect x? when x/[A]i < 0.05
quadratic formula (-b ± sqrt(b² - 4ac)) / (2a)
Reactant Quotient (Q) expressed in same way as equilibrium constant, but used when system isn't at equilibrium
Le Chatlier's Principle if equilibrium is stressed, the system will shift in response and will re-establish equilibrium
Increase temp (change in equilib) to left if exothermic (heat is product), to right if endothermic
Use catalyst (change in equilib) rxn shifts right, lower Ea
Pressure increase/lower vol. (change in equilib) shifts towards less products
Q vs K values smaller Q favors forward rxn, bigger Q favors reverse rxn
Reversing rxn for K Kforward = 1/Kreverse
Changing conc for K changing coeffocients by x results in constant changing by same factor (K)^x
two equilib constants tg multiply by eachother for final
gibbs free energy max amount of energy released by rxn at a constant temp/pressure
Gibbs free energy values G<0 favors products(K>1), G>0 favors reactants(K<1)
pH negative log of hydronium ion concentration (acidic <7, basic >7)
Strong Acids HCl, HBr, HI, HNO3, H2SO4, HClO4, HClO3
Strong bases LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
Percent ionization [H3O+]e/[HA]i x100 Increase with Ka and decreases with increasing [HA]
Created by: user-2004513
 

 



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