The diagram shows the almost complete dissociation of a strong acid in aqueous solution
pH is the negative log of the concentration of H+/H3O+ ions and can be calculated if the concentration of the strong acid is known using the stoichiometry of the reaction
The diagram shows the almost complete dissociation of a weak acid in aqueous solution
Acid & equilibrium position table
The position of the equilibrium is so far over to the right that you can represent the reaction as an irreversible reaction
The diagram shows the almost complete dissociation of a strong base in aqueous solution
The diagram shows the almost complete dissociation of a weak base in aqueous solution
Base & equilibrium position table
Hydrogen ions in aqueous solutions can be written as either as H3O+ or as H+ however, if H3O+ is used, H2O should be included in the chemical equation:HCl(g) → H+(aq) + Cl-(aq)orHCl(g) + H2O(l) → H3O+(aq) + Cl-(aq) Remember that some acids are both strong and weak acids – for example, H2SO4 (sulfuric acid) has two hydrogen ions that can ionise.H2SO4 acts as a strong acid: H2SO4 → H+ + SO4-HSO4- acts as a weak acid: HSO4-⇌ H+ + SO42- Also, don't forget that the terms strong and weak acids and bases are related to the degree of dissociation and not the concentration.The appropriate terms to use when describing concentration are dilute and concentrated.
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