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.
An acid dissociation constant, Ka, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions. The equilibrium can be written symbolically as: HA A− + H+,
In water solutions an acid or a base is diluted depending on the amount of water. But when water is added with an acid or base it also undergoes a condition called chemical equilibrium. For more information on chemical equilibrium check some more wikianswers or look it up on google :L
Suppose: B- is symbol for any (soluble) base.Equilibrium of a base when diluted in water:B- + H2O HB + OH-Equilibrium constant:Keq = [HB] * [OH-] / [B-] * [H2O]The base dissociation contant is defined by:KB = [HB]*[OH-]/[B-]So, KB = Keq*[H2O] = Keq*55.6 mol/L
Water ampholytic (acid+base) equilibrium: H2O + H2O <--> H3O+ + OH-
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.
An acid dissociation constant, Ka, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions. The equilibrium can be written symbolically as: HA A− + H+,
An acid-base equilibrium is the state in whic the concentrations of acidic and basic ions in a solution neutralize each other.
In water solutions an acid or a base is diluted depending on the amount of water. But when water is added with an acid or base it also undergoes a condition called chemical equilibrium. For more information on chemical equilibrium check some more wikianswers or look it up on google :L
Determination of the Dissociation Constant and Molar Mass for a Weak AcidAbstract: We will determine Ka and the molar mass for an unknown weak acid by using a pH meter to record the pH at intervals during the titration with sodium hydroxide. The titration curve and its first derivative will be plotted to establish the equivalence point. Introduction The strength of an acid is defined by its ability to donate a proton to a base. For many common acids, we can quantify acid strength by expressing it as the equilibrium constant for the reaction in which the acid donates a proton to the standard base, water, as shown in the equations below: HA + H2O Û H3O+ + A-, for H3CCOOH: H3CCOOH + H2O Û H3O+ + H3CCOO - The equilibrium constant for a reaction of this type is called the Acid Dissociation Constant, "Ka", for the acid HA Determination of the Dissociation Constant and Molar Mass for a Weak AcidAbstract: We will determine Ka and the molar mass for an unknown weak acid by using a pH meter to record the pH at intervals during the titration with sodium hydroxide. The titration curve and its first derivative will be plotted to establish the equivalence point. Introduction The strength of an acid is defined by its ability to donate a proton to a base. For many common acids, we can quantify acid strength by expressing it as the equilibrium constant for the reaction in which the acid donates a proton to the standard base, water, as shown in the equations below: HA + H2O Û H3O+ + A-, for H3CCOOH: H3CCOOH + H2O Û H3O+ + H3CCOO - The equilibrium constant for a reaction of this type is called the Acid Dissociation Constant, "Ka", for the acid HA Determination of the Dissociation Constant and Molar Mass for a Weak AcidAbstract: We will determine Ka and the molar mass for an unknown weak acid by using a pH meter to record the pH at intervals during the titration with sodium hydroxide. The titration curve and its first derivative will be plotted to establish the equivalence point. Introduction The strength of an acid is defined by its ability to donate a proton to a base. For many common acids, we can quantify acid strength by expressing it as the equilibrium constant for the reaction in which the acid donates a proton to the standard base, water, as shown in the equations below: HA + H2O Û H3O+ + A-, for H3CCOOH: H3CCOOH + H2O Û H3O+ + H3CCOO - The equilibrium constant for a reaction of this type is called the Acid Dissociation Constant, "Ka", for the acid HA
Jordan J. Cohen has written: 'Acid-base' -- subject(s): Acid-base equilibrium, Acid-base imbalances
Suppose: B- is symbol for any (soluble) base.Equilibrium of a base when diluted in water:B- + H2O HB + OH-Equilibrium constant:Keq = [HB] * [OH-] / [B-] * [H2O]The base dissociation contant is defined by:KB = [HB]*[OH-]/[B-]So, KB = Keq*[H2O] = Keq*55.6 mol/L
Edward Jasper King has written: 'Acid-base equilibria' -- subject(s): Acid-base equilibrium
Poul Kildeberg has written: 'Clinical acid-base physiology' -- subject(s): Acid-base equilibrium, Pediatrics
Wilhelm R. Frisell has written: 'Acid-base chemistry in medicine' -- subject(s): Acid-base equilibrium
Water ampholytic (acid+base) equilibrium: H2O + H2O <--> H3O+ + OH-
Peter A. Stewart has written: 'How to Understand Acid-Based' 'How to understand acid-base' -- subject(s): Acid-base equilibrium, Body fluids, Electrolyte metabolism