Understanding acids and bases is crucial in chemistry. Acids like HCl donate protons, while bases like NaOH accept them. The strength of these substances is shown by their dissociation in water, affecting the pH scale. Weak acids and bases partially dissociate, creating an equilibrium crucial for pH levels. Equilibrium constants, Ka and Kb, quantify their dissociation, essential for calculating pH and conducting titrations.
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Acids donate protons while bases accept protons in aqueous solutions
Equilibrium of Weak Acids and Bases
Weak acids and bases exhibit partial dissociation in solution, creating an equilibrium between the undissociated species and ions
pH Scale
The pH scale measures the concentration of hydrogen ions in a solution, with lower values indicating higher acidity and higher values indicating basicity
Equilibrium Constants (Ka and Kb)
Ka and Kb values reflect the strength of weak acids and bases, with larger values indicating stronger species
The pH of a solution containing a weak acid or base can be calculated using the equilibrium constant and initial concentration, and titration can be used to determine the concentration of an acid or base
Acetic acid and ammonia are examples of weak acids and bases, respectively, commonly used in everyday products
The properties of weak acids and bases, such as pH and reactivity, are utilized in various industries and processes
00
Substances like hydrochloric acid (______) and acetic acid (______) are known to donate protons in aqueous solutions.
HCl
CH3COOH
01
In contrast to acids, compounds such as sodium hydroxide (______) and ammonia (______) are known to accept protons.
NaOH
NH3
02
Weak acid equilibrium representation
HA(aq) ⇌ H+(aq) + A−(aq); shows partial dissociation of weak acid into ions.
