2.3.1 Acids and bases

• What ions do acids produce in water according to the Arrhenius definition?

  Hydronium ions (H3O+)
• According to the Arrhenius definition, acids have a pH less than 7
• What key ion is associated with acids in the Brønsted-Lowry definition?

  Proton (H+)
• Match the definitions with their corresponding theories:

  Arrhenius ↔️ Acids produce H3O+, bases produce OH- in water

  Brønsted-Lowry ↔️ Acids donate protons, bases accept protons
• The Brønsted-Lowry definition works in both aqueous and non-aqueous solutions
• The key ions in the Arrhenius definition are H3O+ and OH-
• The Brønsted-Lowry definition works in both aqueous and non-aqueous solutions.
• Strong acids completely ionize in water to produce a high concentration of hydronium ions.

  True
• Weak acids only partially ionize in water, producing a lower concentration of hydronium ions.
• Weak acids have a high hydronium ion concentration in water.

  False
• What ion do strong bases release in high concentration when dissolved in water?

  OH-
• The pH scale ranges from 0 to 14, with 7 being neutral
• The Arrhenius definition states that acids produce hydronium ions in water.


  True
• What does the Brønsted-Lowry definition consider a base to be?

  Proton acceptor
• The Brønsted-Lowry definition extends to reactions in non-aqueous solutions.
• The Arrhenius definition works in both aqueous and non-aqueous solutions

  False
• In what type of solutions does the Brønsted-Lowry definition apply?

  Aqueous and non-aqueous
• Why is the Brønsted-Lowry definition considered more general than the Arrhenius definition?

  Focuses on proton transfer
• What is an example of a strong acid?

  Hydrochloric acid (HCl)
• What happens to weak acids in water?

  They partially ionize
• Match the acid property with its type:

  Strong Acids ↔️ Complete ionization

  Weak Acids ↔️ Partial ionization
• Strong bases release a high concentration of hydroxide ions in water.
• What happens when sodium hydroxide (NaOH) is added to water?

  Releases many OH- ions
• Arrange the pH levels from most acidic to most basic:

  1️⃣ pH 0

  2️⃣ pH 7

  3️⃣ pH 14
• The relationship between pH and pOH is pH + pOH = 14</latex>


  True
• What is the pOH of a solution with a pH of 10?

  4
• The relationship between pH and pOH is expressed as pH + pOH = 14
• What is the formula to calculate pOH given the [OH-] concentration?

  $pOH =$$- \log[OH^ - ]$
• In a solution with pH 5, what is the pOH?

  9
• For a solution with a pH of 10, the pOH is 4.


  True
• The sum of pH and pOH is always 14 at standard temperature.

  True
• The pOH is calculated by taking the negative logarithm of the hydroxide ion concentration
• If a solution has [OH-] = 1.0 x 10^-9 M, its pOH is 9.0.


  True
• Steps to calculate pOH given [OH-]

  1️⃣ Determine the [OH-] concentration

  2️⃣ Take the negative logarithm of the [OH-] concentration

  3️⃣ Use the relationship pH + pOH = 14 to calculate the pH
• What ions do bases produce in water according to the Arrhenius definition?

  Hydroxide ions (OH-)
• According to the Brønsted-Lowry definition, bases are proton donors.

  False
• The Arrhenius definition requires acids and bases to be dissolved in water
• Conjugate acid-base pairs occur when an acid donates a proton and a base accepts a proton.


  True
• What type of solvent is required for the Arrhenius definition of acids and bases?

  Aqueous only
• The Arrhenius definition defines acids as substances that produce hydronium ions in water.

  True