Acids & Bases

    Cards (57)

    • What is a Bronsted-Lowry acid?
      Proton donor
    • What is a Bronsted-Lowry base?
      Proton acceptor
    • What ion causes a solution to be acidic?
      H+ (hydrogen ion)
    • What is the formula for the oxonium ion?
      H3O+
    • What ion causes a solution to be alkaline?
      OH- (hydroxide ion)
    • Write an equation for the ionisation of water.
      2H2O (l) ⇌ H3O+ (aq) + OH- (aq)
    • How is Kw derived from the ionisation of water?
      Kw = [H3O+][OH-]
    • What is the value of Kw at 298K?
      1.0 x 10^-14
    • What physical factor affects the value of Kw?
      Temperature
    • How does increasing temperature affect Kw?
      Kw increases and pH decreases
    • Why is pure water still neutral?
      [H+] = [OH-]
    • What is the expression for pH in terms of H+?
      pH = -log10[H+]
    • What is the relationship between pH and concentration of H+?
      Lower pH = higher concentration of H+
    • If two solutions have a pH difference of 1, what is the difference in [H+]?
      A factor of 10
    • How do you find [H+] from pH?
      [H+] = 10^-pH
    • How do you find [OH-] from pH at 298K?
      Use Kw to calculate [OH-]
    • What is different when finding [H+] from diprotic and triprotic acids?
      Multiply concentration by number of protons
    • How do you calculate the pH of a strong alkaline solution?
      Use Kw to calculate [H+]
    • Define a strong acid.
      Fully dissociates in water
    • Define a strong base.
      Fully dissociates in water
    • What is the difference between concentrated and strong?
      Concentrated refers to molarity, strong to dissociation
    • What is a weak acid and a weak base?
      Do not fully dissociate in water
    • What is Ka?
      Acid dissociation constant
    • How would you work out the pH of a weak acid?
      Use Ka and pH = -log[H+]
    • What is a titration?
      Adding known acid/base to unknown concentration
    • What is the purpose of an indicator in titration?
      To show that neutralization has occurred
    • What is the equivalence point in titration?
      Exact volume of base neutralizes acid
    • What generally happens to the pH around the equivalence point?
      pH changes rapidly
    • What are the titration curves for different acid-base combinations?
      • Strong acid with strong base: steep curve
      • Strong acid with weak base: gradual rise
      • Weak acid with weak base: shallow curve
      • Weak acid with strong base: initial rise, then steep
    • What is the significance of the equivalence point in titration?
      • Indicates complete neutralization
      • Essential for accurate concentration determination
      • Guides the choice of indicator
    • What is the titration curve for a weak acid with a weak base?
      It shows gradual pH changes.
    • What is the titration curve for a weak acid with a strong base?
      It shows a steep increase in pH.
    • What is the equivalence point in titration?
      The exact volume of base neutralizing acid.
    • What happens to the pH around the equivalence point?
      There is a large and rapid change in pH.
    • How do you calculate the concentration of a reactant?
      Use mols and volume from the balanced equation.
    • What is the end point in titration?
      The volume when the indicator changes color.
    • What are the properties of a good indicator for a reaction?
      • Sharp color change (not gradual)
      • End point matches equivalence point
      • Distinct color change for clarity
    • Which indicator is used for a strong acid-strong base titration?
      Phenolphthalein or methyl orange.
    • Which indicator is used for a strong acid-weak base titration?
      Methyl orange.
    • Which indicator is used for a strong base-weak acid titration?
      Phenolphthalein.
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