Chapter 10 Quiz: Acids and Bases in Our Environment

What is the taste commonly associated with acids?

• Bitter

• Sweet

• Sour

• Salty

According to Brønsted–Lowry theory, which substance acts as a base in the reaction: NH₃ + H₂O ⇌ NH₄⁺ + OH⁻?

• NH₃

• H₂O

• NH₄⁺

• OH⁻

Identify the acid and base in the reaction: HCl + H₂O → Cl⁻ + H₃O⁺.

• HCl is the base, H₂O is the acid

• HCl is the acid, H₂O is the base

• Both are acids

• Both are bases

What is true about amphoteric substances like water?

• They always donate protons

• They always accept protons

• They can act as acids or bases depending on the situation

• They are neutral and never react

Using the Lewis definition, CO₂ behaves as:

• A Lewis base because it donates an electron pair

• A Lewis acid because it accepts an electron pair

• A neutral molecule with no acid-base behavior

• A Bronsted-Lowry acid because it donates a proton

Which of the following is a strong acid?

• Acetic acid

• Hydrochloric acid

• Citric acid

• Carbonic acid

What determines the strength of an acid or base?

• Its pH level

• Its molarity

• The extent to which it dissociates in water

• Its color

Why do strong acids conduct electricity better than weak acids?

• They are always more concentrated

• They release more ions in solution

• They produce bubbles

• They are always hotter

Which statement about corrosive ability is true?

• Stronger acids are always more corrosive

• Corrosiveness depends on the number of hydrogen atoms

• Corrosiveness is based on concentration

• Weak acids can never be corrosive

Predict the outcome: A solution of a weak acid is made highly concentrated. What might happen?

• It becomes a strong acid

• It remains weak but becomes more corrosive

• It loses all its acidity

• It starts conducting electricity like a metal