HX ---> H+ + X-
Keq = [H+][X-]/[HX]
C + O ==> COKeq = [CO]/[C][O]
The only reaction and equilibrium takes place in pure water is the dissociation to hydroxonium and hydroxil ions. So they remain in same concentrations independent from temperature.
In neutralisation reactions H+ and OH- ions come from the dissociation of water, H2O, which is part of the solution.Water dissociates in equilibrium, shown as:H2O(l) H+(aq) + OH-(aq)
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
Water + Carbon dioxide Carbonic acidH2O + CO2 H2CO3 equilibrium
Keq = [H2O][CO] [H2][CO2]
C + O ==> COKeq = [CO]/[C][O]
The only reaction and equilibrium takes place in pure water is the dissociation to hydroxonium and hydroxil ions. So they remain in same concentrations independent from temperature.
dissociation reaction
The concentration of OH- decreases as the concentration of H+ increases. This is beacause there is an equilibrium H2O <-> H+ + OH- and therefore the [H+][OH-] is a constant
Constant data and constant functions.
A constant is a variable that does not change. The correct term is constant variable.
In neutralisation reactions H+ and OH- ions come from the dissociation of water, H2O, which is part of the solution.Water dissociates in equilibrium, shown as:H2O(l) H+(aq) + OH-(aq)
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
A constant object is one that, once initialized, never changes value.