Exploring Acid-Base Theories

What is the Bronsted-Lowry definition of an acid?

• A Bronsted-Lowry acid is a proton acceptor.

• A Bronsted-Lowry acid is a hydroxide donor.

• A Bronsted-Lowry acid is a salt.

• A Bronsted-Lowry acid is a proton donor.

How does the Bronsted-Lowry theory differ from the Arrhenius theory?

• The Arrhenius theory is broader, including non-aqueous solutions.

• The Bronsted-Lowry theory is broader, defining acids as proton donors and bases as proton acceptors, while the Arrhenius theory is limited to aqueous solutions.

• The Bronsted-Lowry theory only applies to strong acids and bases.

• The Arrhenius theory defines acids as proton donors and bases as proton acceptors.

Define a Lewis acid and provide an example.

• Carbon dioxide (CO2)

• An example of a Lewis acid is aluminum chloride (AlCl3).

• Water (H2O)

• Sodium chloride (NaCl)

What is a Lewis base and how does it interact with a Lewis acid?

• A Lewis base reacts with a Lewis acid to form a gas.

• A Lewis base and a Lewis acid do not interact chemically.

• A Lewis base accepts an electron pair from a Lewis acid.

• A Lewis base donates an electron pair to a Lewis acid, which accepts the electron pair.

Explain the process of acid-base neutralization.

• Acid-base neutralization only produces carbon dioxide and water.

• The process involves mixing two acids to create a stronger acid.

• Acid-base neutralization produces water and a salt from the reaction of an acid and a base.

• Neutralization results in the formation of only a gas without any liquid products.

What are the products of a typical acid-base neutralization reaction?

• Hydrogen and oxygen

• Carbon dioxide and ammonia

• Water and salt

• Sodium and chlorine

How is the pH scale defined and what does it measure?

• The pH scale is used to measure the density of a liquid.

• The pH scale measures the acidity or alkalinity of a solution.

• The pH scale indicates the concentration of dissolved oxygen in water.

• The pH scale measures temperature changes in a solution.

Calculate the pH of a solution with a hydrogen ion concentration of 0.001 M.

• 3

• 5

• 2

• 4

What is the relationship between pH and pOH?

• pH + pOH = 14

• pH is the same as pOH

• pH + pOH = 7

• pH is a measure of acidity only

How do strong acids differ from weak acids in terms of ionization?

• Weak acids ionize more than strong acids.

• Strong acids partially ionize, weak acids fully ionize.

• Strong acids fully ionize, weak acids partially ionize.

• Both strong and weak acids fully ionize.