At a constant 100 C and 1 ATM ambient pressure, I believe it should be 1 as the gaseous and liquid phases would be equally favored. This is due to the fact that the vapor pressure of liquid water at 100 C is 1 ATM.
1x10^-14
Kc is the constant for concentration and Kw is the constant for water. Kc[h20] = [OH-][H+] which becomes Kw= [OH-][H+]
Kw is called the water autoprotolysis constant or water autoionization constant
The information an acid or base equilibrium constant gives is that the acidity and base levels are equal to the equilibrium constant multi[plied by the water concentration.
Ion product constant is essentially when something reaches equilibrium. Such as in the case of water. When water reaches its ion product constant it becomes both a base and an acid, reaching equilibrium.
1.0*10^-14 No Units
Kw is the ionisation constant for water at 25°C which value is 1.0x10^-14. (chemistry)In water at any pH the equilibrium state Kw is defined by and equal to the 'ion product':Kw = [H3O+]*[OH-] = 1.0*10-14at room temperature 25°C
Kc is the constant for concentration and Kw is the constant for water. Kc[h20] = [OH-][H+] which becomes Kw= [OH-][H+]
Kw is called the water autoprotolysis constant or water autoionization constant
The information an acid or base equilibrium constant gives is that the acidity and base levels are equal to the equilibrium constant multi[plied by the water concentration.
Ion product constant is essentially when something reaches equilibrium. Such as in the case of water. When water reaches its ion product constant it becomes both a base and an acid, reaching equilibrium.
Yes, it is an equilibrium constant, ONLY depending on the kind of reaction (Kw for water protolysis) and on temperature (according to Arrhenius) and never, NEVER on concentrations of its reactants and products:that is just why it is called a 'C O N S T A N T'
solubility product constant.
The ionization constant of water at 250C, its value is 1x10-14 A: ion-product constant of water.
If their concentrations are multiplied with one other the product equals the water constant Kw:a kind of 'equilibrium constant' of the 'water equilibrium' reactions and vice verse: *)[H+]*[OH-] = Kw = 1.0*10-14or in negative log10 value's: (analogs of pH = -log[H+] ) pH + pOH = pKw = 14.0*) This equilibrium state is reached very quickly, so in any watery solution this is always a constant value. [H+] and [OH-] are always depending on each other: If you add acid (H+) then H+ goes up AND SO OH- goes down!H+ + OH- H2O
No, the equilibrium constant is independent of concentration as long as the ratio of products and reactants remains as is. It can be effected by anything that would influence the ratio of products and reactants, such as changes in temperature or the addition of a catalysis.
1.0*10^-14 No Units
Kc is the equilibrium constant of a chemical reaction; Kp is the equilibrium constant of a chemical reaction at constant pressure.