8.1 Introduction to Acids and Bases

• Acids donate protons (H⁺) according to the Bronsted-Lowry theory

  True
• Arrhenius acids increase the concentration of hydrogen ions (H⁺) when dissolved in water
• The Brønsted-Lowry theory defines acids as proton donors
• Acids and bases are classified as strong or weak based on their extent of dissociation
• Match the characteristics with Arrhenius acids or bases:

  Arrhenius Acids ↔️ H⁺ concentration increases

  Arrhenius Bases ↔️ OH⁻ concentration increases
• The Arrhenius theory cannot explain the basic properties of substances like ammonia
• The Brønsted-Lowry theory defines acids and bases more broadly than the Arrhenius theory.
• Match the type of acid or base with its dissociation in water and an example:

  Strong Acid ↔️ Completely dissociates; HCl

  Strong Base ↔️ Completely dissociates; NaOH

  Weak Acid ↔️ Partially dissociates; CH₃COOH

  Weak Base ↔️ Partially dissociates; NH₃
• A conjugate acid-base pair differs by the presence or absence of a proton (H⁺).


  True
• Amphiprotic substances can act as both proton donors and proton acceptors.


  True
• What is the relationship between pH and pOH?

  pH + pOH = 14
• The sum of pH and pOH is always equal to 14.
• Give three examples of common acids.

  HCl, H₂SO₄, CH₃COOH
• Common examples of acids include HCl, H₂SO₄, and CH₃COOH
• Match the type of acid/base with its example:

  Strong Acid ↔️ HCl

  Strong Base ↔️ NaOH

  Weak Acid ↔️ CH₃COOH

  Weak Base ↔️ NH₃
• The Brønsted-Lowry theory can explain the basic properties of ammonia in aqueous solutions.


  True
• Common examples of amphiprotic substances include water and bicarbonate ions.
• pOH is calculated using the formula: pOH = -log[OH⁻].
• What does pH measure?

  Hydrogen ion concentration
• What does pOH measure?

  Hydroxide ion concentration
• What is the pH of blood?

  7.4
• What do strong acids release when they dissociate in water?

  All H⁺
• What is the self-ionization of water?

  Water acting as both acid and base
• What is the value of \(K_w\) at 25°C?

  1.0 x 10⁻¹⁴
• Common examples of acids include HCl, H₂SO₄, and CH₃COOH
• The Arrhenius theory can explain the basic properties of ammonia

  False
• Brønsted-Lowry bases accept protons (H⁺).


  True
• The Brønsted-Lowry theory can explain the basic properties of ammonia.


  True
• According to the Brønsted-Lowry theory, bases accept protons
• The Arrhenius theory defines acids based on their ability to increase the concentration of H⁺
• Arrhenius acids cause the concentration of hydroxide ions (OH⁻) to decrease
• Compare and contrast Arrhenius acids and bases based on their behavior in water:

  1️⃣ Arrhenius Acids increase H⁺ concentration

  2️⃣ Arrhenius Bases increase OH⁻ concentration

  3️⃣ Arrhenius Acids cause OH⁻ concentration to decrease

  4️⃣ Arrhenius Bases cause H⁺ concentration to decrease
• Brønsted-Lowry acids are substances that donate protons (H⁺).


  True
• An acid donates a proton to form its conjugate base.
• Match the category with its action and an example:

  Amphiprotic ↔️ Donates and accepts protons; H₂O

  Acid ↔️ Donates protons; HCl

  Base ↔️ Accepts protons; NaOH
• Blood has a pH around 7.4, indicating it is slightly basic.


  True
• What action defines a Brønsted-Lowry acid?

  Donates protons
• According to the Brønsted-Lowry theory, acids are substances that donate protons
• Arrhenius acids increase the concentration of H⁺ ions in water.


  True
• Brønsted-Lowry acids donate protons.


  True