strong acids and bases

• What do acid-base equilibria involve?

  The transfer of protons between substances
• How are substances classified as acids or bases in the Brønsted-Lowry theory?

  Based on their interaction with protons
• What is a Brønsted-Lowry acid?

  A proton donor
• Give an example of a Brønsted-Lowry acid.

  Ammonium ions (NH$_4^+$)
• What is a Brønsted-Lowry base?

  A proton acceptor
• Give an example of a Brønsted-Lowry base.


  Hydroxide ions (OH$^-$)
• How is a strong acid defined?

  An acid that completely dissociates to ions when in solution with pH 3-5
• What is the pH range of a strong acid?

  pH 3-5
• How is a weak acid defined?

  An acid that only slightly dissociates when in solution with pH 0-1
• What is the pH range of a weak acid?

  pH 0-1
• What does pH measure?

  Acidity and alkalinity
• What type of scale is pH?

  A logarithmic scale from 0 to 14
• What does a pH of 0 indicate?

  An acidic solution with a high concentration of H$^+$ ions
• What does a pH of 14 indicate?

  A basic solution with a low concentration of H$^+$ ions
• How can the concentration of H$^+$ ions be determined?


  Using the pH value
• What is the ionic product of water?

  Water slightly dissociates to ions as an equilibrium with its own equilibrium constant, K$w$
• How does the value of K$w$ change?


  It changes with temperature
• What type of reaction is the forward reaction in the equilibrium of water?

  Endothermic
• What happens to the concentration of H$^+$ ions as the temperature of water increases?


  More H$^+$ ions are produced, making the water more acidic
• What are the key concepts of Brønsted-Lowry acids and bases?

  • Brønsted-Lowry acid: proton donor
  • Brønsted-Lowry base: proton acceptor
  • Acid-base equilibria involve proton transfer
• What are the definitions of strong and weak acids and bases?

  • Strong acid: completely dissociates in solution (pH 3-5)
  • Weak acid: slightly dissociates in solution (pH 0-1)
  • Strong base: has pH 12-14
  • Weak base: has pH 9-11
• What is the relationship between pH and H$^+$ ion concentration?


  • pH measures acidity and alkalinity
  • pH scale: 0 (acidic) to 14 (basic)
  • H$^+$ concentration can be determined from pH
• What is the significance of the ionic product of water?

  • Water dissociates into ions
  • Equilibrium constant K$w$ at 25°C is 1 x 10$^{-14}$
  • K$w$ changes with temperature
• How does temperature affect the acidity of water?

  • Increased temperature favors the forward reaction
  • More H$^+$ ions are produced
  • Water becomes more acidic as temperature increases