Allery Acids and bases

Cards (156)

  • What is the significance of the hydronium ion in acid solutions?
    It makes the solution acidic
  • What is the formula for the hydronium ion?
    H<sub>3</sub>O<sup>+</sup>
  • What do Bronsted-Lowry acids do?
    They donate protons
  • What do Bronsted-Lowry bases do?
    They accept protons
  • What is a characteristic of strong acids?
    They dissociate almost completely
  • What is a characteristic of weak acids?
    They dissociate poorly
  • What do strong bases do in solution?
    They produce a lot of OH<sup>-</sup> ions
  • What is the equilibrium position for weak acids?
    • The backward reaction is favored
    • Few H<sup>+</sup> ions produced
  • What is the equilibrium position for strong acids?
    • The forward reaction is favored
    • Many H<sup>+</sup> ions produced
  • What happens when acids and bases react according to Bronsted-Lowry theory?
    Protons are exchanged
  • What is the ionic product of water denoted as?
    K<sub>w</sub>
  • What is the value of K<sub>w</sub> at a given temperature?
    1 x 10<sup>-14</sup> mol<sup>2</sup> dm<sup>-6</sup>
  • What does pH measure?
    The concentration of H<sup>+</sup> ions
  • What is the formula to calculate pH?
    pH = -log<sub>10</sub>[H<sup>+</sup>]
  • If a solution has a pH of 0, how is it classified?
    Very acidic
  • If a solution has a pH of 14, how is it classified?
    Very basic
  • What is the relationship between pH and acidity?
    • Lower pH indicates higher acidity
    • Higher pH indicates lower acidity
  • How do strong acids and weak acids differ in terms of dissociation?
    • Strong acids dissociate completely
    • Weak acids dissociate poorly
  • How do strong bases and weak bases differ in terms of dissociation?
    • Strong bases dissociate completely
    • Weak bases dissociate poorly
  • What is the significance of equilibrium in acid-base reactions?
    • Determines the concentration of products and reactants
    • Affects the strength of acids and bases
  • What does pH measure in a solution?
    Concentration of H+ ions
  • Why is the pH scale logarithmic?
    It converts small numbers into manageable values
  • What is the pH of a neutral substance?
    7
  • What does a pH of 0 indicate?
    Very acidic substance
  • What is the equation to calculate pH?
    pH = -log<sub>10</sub>[H+]
  • How do you calculate the pH of hydrochloric acid with a concentration of 0.03 moles per cubic meter?
    pH = -log<sub>10</sub>(0.03)
  • What does a pH of 1.5 suggest about hydrochloric acid?
    It indicates a strong acid
  • How can you calculate the concentration of H+ ions from pH?
    Use H+ = 10<sup>-pH</sup>
  • What is the concentration of H+ ions in nitric acid with a pH of 1.7?
    0.0198 moles per cubic meter
  • What is the assumption made about strong acids like hydrochloric acid?
    They dissociate fully in solution
  • How do you calculate the pH of 0.25 moles per cubic meter of hydrochloric acid?
    pH = -log<sub>10</sub>(0.25)
  • What is a diprotic acid?
    An acid that produces two H+ ions per molecule
  • How do you calculate the pH of 0.25 moles per cubic meter of sulfuric acid?
    pH = -log<sub>10</sub>(0.5)
  • What is the relationship between strong bases and their dissociation?
    Strong bases dissociate fully in solution
  • How do you calculate the pH of sodium hydroxide with a concentration of 0.15 moles per cubic meter?
    Use KW to find H+ concentration
  • What is the value of KW at 298 Kelvin?
    1 x 10<sup>-14</sup> moles squared per cubic meter
  • How do you find the concentration of H+ ions from the concentration of OH- ions?
    Use H+ = KW / [OH-]
  • What is the acid dissociation constant (Ka)?
    It measures the strength of weak acids
  • How do you calculate the pH of a weak acid like ethanoic acid?
    Use the Ka expression for weak acids
  • What is the Ka expression for a weak acid?
    Ka = [H+]<sup>2</sup> / [HA]