Strength of Acids and Bases

The strength of an acid or base refers to its ability to dissociate into ions in solution. Acids and bases can be categorized as strong or weak based on the extent of their ionization:

A. Strong Acids and Bases: 
 - Strong Acids: Strong acids completely dissociate into ions in solution, releasing all of their hydrogen ions (\(H^+\)). Examples include hydrochloric acid (\(HCl\)), sulfuric acid (\(H_2SO_4\)), and nitric acid (\(HNO_3\)).
     \[ HCl \rightarrow H^+ + Cl^- \]
     \[ H_2SO_4 \rightarrow 2H^+ + SO_4^{2-} \]
     \[ HNO_3 \rightarrow H^+ + NO_3^- \]
   

- Strong Bases: Strong bases dissociate completely into hydroxide ions (\(OH^-\)) and a cation in solution. Examples include sodium hydroxide (\(NaOH\)) and potassium hydroxide (\(KOH\)).
     \[ NaOH \rightarrow Na^+ + OH^- \]
     \[ KOH \rightarrow K^+ + OH^- \]

B. Weak Acids and Bases:
 - Weak Acids: Weak acids only partially dissociate in solution, resulting in an equilibrium between the undissociated acid molecules and the ions formed. Examples include acetic acid (\(CH_3COOH\)) and carbonic acid (\(H_2CO_3\)).
     \[ CH_3COOH \rightleftharpoons CH_3COO^- + H^+ \]
     \[ H_2CO_3 \rightleftharpoons HCO_3^- + H^+ \]
 

- Weak Bases: Weak bases similarly undergo partial dissociation in solution, forming hydroxide ions and the conjugate acid. Ammonia (\(NH_3\)) is an example of a weak base.
     \[ NH_3 + H_2O \rightleftharpoons NH_4^+ + OH^- \]

C. Relationship with Dissociation Constants:
   - For weak acids and bases, the extent of dissociation is quantified by their dissociation constants (\(K_a\) for acids and \(K_b\) for bases).
   - The larger the value of \(K_a\) or \(K_b\), the stronger the acid or base, as it indicates a greater extent of dissociation.
   - The dissociation constant expression for a weak acid is given by:
     \[ K_a = \frac{[H^+][A^-]}{[HA]} \]
   - Similarly, for a weak base, the dissociation constant expression is:
     \[ K_b = \frac{[BH^+][OH^-]}{[B]} \]

Understanding the strength of acids and bases is essential for predicting their behavior in chemical reactions and determining their suitability for various applications.

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