Chemistry Quiz on Acids and Bases

What is the pH of a 0.0025 M solution of hydrochloric acid?

• 2.6

• 7.0

• 1.2

A BrØnsted-Lowry base is defined as a substance that ___.

• increases [H+] when placed in H2O

• Decrease [H+] when placed in H2O

• increase [OH-] when placed in H2O

• acts as a proton acceptor

• acts as a proton donor

What is the conjugate base of OH-?

• O2

• O-

• O2-

• H2O+

• H2O

A substance that is capable of acting as both an acid and as a base is _______.

• saturated

• Autosoma

• miscible

• amphoteric

• Conjugated

A BrØnsted-Lowry acid is defined as a substance that _______.

• acts as a proton acceptor

• decrease [H+] when placed in H2O

• increase [H+] when placed in H2O

• acts as a proton donor

• Increases [OH-] when placed in H2O

What is the conjugate acid of NH3?

• NH4OH

• NH2+

• NH4+

• NH3

• NH2+

What is the expression for the ion-product constant of water (Kw) at 25°C?

• Kw = [H₃O⁺] / [OH⁻]

• Kw = [H₃O⁺] × [OH⁻]

• Kw = [H₂O]²

• Kw = [H⁺] + [OH⁻]

In pure water at 25°C, what are the concentrations of H₃O⁺ and OH⁻ ions?

• [H₃O⁺] = 1.0 × 10⁻⁷ M; [OH⁻] = 1.0 × 10⁻⁷ M

• [H₃O⁺] = 1.0 × 10⁻⁶ M; [OH⁻] = 1.0 × 10⁻⁸ M

• [H₃O⁺] = 1.0 × 10⁻⁸ M; [OH⁻] = 1.0 × 10⁻⁶ M

• [H₃O⁺] = 1.0 × 10⁻¹⁴ M; [OH⁻] = 1.0 M

What does it mean when a substance is described as amphoteric?

• It can only donate protons.

• It can only accept protons.

• It can act as both an acid and a base.

• It is neutral and does not participate in acid-base reactions.

If the concentration of H₃O⁺ in a solution is 1.0 × 10⁻⁵ M at 25°C, what is the concentration of OH⁻?

• 1.0 × 10⁻⁵ M

• 1.0 × 10⁻⁹ M

• 1.0 × 10⁻⁷ M

• 1.0 × 10⁻¹⁴ M