Acids vs Bases, pH

Which statement describes an Arrhenius acid?

• Substance that produces an H⁺ ion when dissolved in water

• Substance that accepts an H⁺ ion

• Substance that produces an OH^- ion when dissolved in water

• Substance that accepts an OH^- ion

Students performed a lab where they measured hydrogen ion concentration after pouring four

different acids into separate beakers containing 200 mL of water. The table shows [H⁺] for

each of the resulting solutions. Based on the information in the table, which is the weakest

acid?

• Solution A

• Solution B

• Solution C

• Solution D

Which of the following is an example of a Bronsted-Lowry base?

• HCl

• NH₃

• H₂O

• NaCl

What is the key characteristic of a strong acid?

• It only partially dissociates in water

• It does not dissociate in water

• It completely ionizes in water

• It is always neutral in solution

Which of the following is an example of a weak acid?

• HCl

• CH₃COOH

• NaOH

• HNO₃

What is the pH of a solution with [H⁺] = 1.3 × 10⁻⁴ M?

• 14

• 3.9

• 4

• 10

If a solution has a pH of 9, what can be said about it?

• It is acidic

• It is neutral

• It is basic

• It has more H⁺ than OH⁻

What happens to the pH of a solution as the concentration of H⁺ increases?

• it becomes more acidic so pH increases

• it becomes more acidic so pH decreases

• It remains the same so pH does not change

• It becomes neutral

Which of the following represents a Bronsted-Lowry acid-base reaction?

• NaOH → Na⁺ + OH⁻

• HCl → H⁺ + Cl⁻

• NH₃ + H₂O ⇌ NH₄⁺ + OH⁻

• H₂O → H⁺ + OH⁻

what formula should you use if you need to calculate pH of a solution but are given the concentration of OH^- ions?

• pH + pOH = 10

• pH + pOH = 14

• pH = 14 - pOH

• pH = - log [OH⁻]