Understanding Acid-Base Concepts

What is the Arrhenius definition of an acid?

• An Arrhenius acid is a substance that decreases the concentration of H+ ions in solution.

• An Arrhenius acid is a substance that increases the concentration of OH- ions in solution.

• An Arrhenius acid is a substance that increases the concentration of H+ ions in solution.

• An Arrhenius acid is a substance that has a pH greater than 7.

Explain the Bronsted-Lowry theory of acids and bases.

• Acids are substances that increase the pH of a solution, while bases decrease it.

• The Bronsted-Lowry theory defines acids as substances that can neutralize bases.

• The Bronsted-Lowry theory states that acids are proton donors and bases are proton acceptors.

• Acids are electron donors and bases are electron acceptors.

What is the Lewis theory of acids and bases?

• The Lewis theory of acids and bases states that acids are electron pair acceptors and bases are electron pair donors.

• Acids are electron pair donors and bases are electron pair acceptors.

• The Lewis theory states that acids release protons and bases absorb protons.

• Acids and bases are defined by their ability to form ionic bonds.

Define pH and its significance in chemistry.

• pH is a scale that measures the density of liquids.

• pH is a scale used to specify the acidity or basicity of an aqueous solution, ranging from 0 (acidic) to 14 (basic), with 7 being neutral.

• pH only applies to solid substances.

• pH is a measure of temperature in a solution.

How do you calculate the pH of a solution?

• pH = 7 - [H+]

• pH = -log10[H+]

• pH = log10[H+]

• pH = [H+] + 14

What is the pH of a neutral solution at 25°C?

• 6

• 5

• 7

• 8

Differentiate between strong and weak acids.

• Strong acids fully ionize in solution; weak acids partially ionize.

• Strong acids are always more corrosive than weak acids.

• Strong acids have a higher pH than weak acids.

• Weak acids do not ionize at all in solution.

Provide an example of a strong acid and a weak acid.

• Strong acid: Hydrofluoric acid (HF), Weak acid: Citric acid (C6H8O7)

• Strong acid: Hydrochloric acid (HCl), Weak acid: Acetic acid (CH3COOH)

• Strong acid: Phosphoric acid (H3PO4), Weak acid: Carbonic acid (H2CO3)

• Strong acid: Sulfuric acid (H2SO4), Weak acid: Nitric acid (HNO3)

What is a buffer solution and its purpose?

• A buffer solution is a type of solvent used for dissolving solids.

• A buffer solution is a mixture that changes color when pH changes.

• A buffer solution is a solution that only contains water and salt.

• A buffer solution is a solution that resists changes in pH upon the addition of small amounts of acid or base.

How does a buffer maintain pH stability?

• A buffer resists changes in pH by neutralizing added acids or bases.

• A buffer changes pH by diluting the solution.

• A buffer only works in acidic environments.

• A buffer increases pH by adding more acids.