Equilibrium constants???

Question

for equilibrium constants, whats the difference between Keq, Ka, Kw... and all that. i thought they were all the same, but idk..

Answer 1

The equilbrium constant has specific names for several classes of reactions as shown below:-

Gas-phase reactions that use units of partial pressure: Kp
Dissociation of water: dissociation constant of water, Kw
Dissociation of acids: acid dissociation constant, Ka
Reaction of bases with water: base hydrolysis constant, Kb
Solubility of precipitates: solubility product, Ksp
Formation of complexes: formation constant, Kf

Answer 2

Keq is the equilibrium constant for a chemical reaction, like CH4 + 2O2 --- CO2 + 2H2O, and Keq would be [CO2][H2O]^2/[CH4][O2]^2. Ka is the constant for an acid dissociation reaction, such as HF --- H+ + F-, and Ka = [H+][F-]/[HF], while Kw is the constant for water, which is 1.00 x 10^-14. It is Kw = [H+][OH-].

Answer 3

Keq is the same for every thing. Ka for acids is Ka = [H=][C2H3O2-]/[HC2H3O2] for acetic acid, HC2H3O2. Kw = [H+][OH-] = 10^-14 for water (w). [H2O] = 1.00 by convention. Kb is for bases like NH4OH. Ksp is solubility product for compounds like BaSO4 or AgCl.

Answer 4

hence, you do no longer use the spectator ions, using actuality they have not have been given to any extent further something to do with the formation and dissociation of FeSCN(2+). For the reaction as written: Keq = [SCN(2+)]/[Fe3+][SCN-]