Acid-Base Equilibria

Which of the following is the correct definition for a strong acid?

• Partially dissociates into ions when dissolved in water and the change is not reversible

• Fully dissociates into ions when dissolved in water and the change is not reversible

• Fully dissociates into ions when dissolved in water and the change is reversible

• Partially dissociates into ions when dissolved in water and the change is reversible

An acid of concentration 1 mol/dm³ has a pH of 2. The acid is diluted to a concentration of 0.01 mol/dm³. What is its new pH?

• 3

• 4

• 2

• 1

which particles are not present in a solution containing dilute hydrochloric acid and ethanoic acid?

• H⁺ ion

• CH₃COO^- ion

• CH₃COOH molecules

• HCl molecule

Which of the following is NOT an acid?

• HCl

• CH₃COOH

• C₂H₆

• H₂SO₄

B, a weak base, can react with water in equilibrium into hydroxide ions and BH⁺ . Which of the following equation represents dissociation of B, a weak base, in water?

• B(aq) + H₂O(l) ⇌ BH⁺(aq) + OH^- (aq)

• B(aq) + H₂O(l) ⇌ BH⁺(aq) + H₃O⁺ (aq)

• B(aq) + H₃O⁺(aq) ⇌ BH⁺(aq) + H₂O(l)

• B(aq) + OH^-(aq) ⇌ BH⁺(aq) + O^2-(aq)

For this reaction :

HA(aq) + H₂O(l) ⇌ H₃O⁺(aq) + A^-(aq)

Which one can act as an acid ?

• HA(aq) and A^-(aq)

• H₂O(l) and H₃O⁺(aq)

• HA(aq) and H₃O⁺(aq)

• H₂O(l) and A^-(aq)

dissociation of weak acid, HA, is represented by following equation :

HA(aq) + H₂O(l) ⇌ H₃O⁺(aq) + A^-(aq)

The equilibrium constant for this reaction is represented by K_a . Which of the following equation represents expression of equilibrium constant, K_a?

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Tags

NGSS.HS-PS1-6

Which one IS TRUE about dissociation of weak acid in water ?

1.[H⁺] ions > [OH^-] ions in weak acid-containing solution

2.The numerical value of Equilibrium constant of dissociation of weak acid, K_a, increase as the temperature decrease

3.It makes light bulb glow very bright

4.pOH > 7 in weak acid-containing solution

• 1, 2, 3 and 4

• 1,2, and 3

• 1,2, and 4

• 2,3 and 4

• 1,3 and 4

Which one IS TRUE about dissociation of weak base in water ?

1.[H⁺] ions = [OH^-] ions in weak base-containing solution

2.The numerical value of Equilibrium constant of dissociation of weak base, K_b, decrease as the temperature decrease

3.Weak base are less dissociated in solution as the amount of concentration of common-ion OH^- in solution increase

4.pH > 7 in weak base-containing solution

• 1, 2, 3, and 4

• 1, 2, and 3

• 2, 3, and 4

• 2 and 4

• 2 and 3

The pH of a solution at 25^ₒC in which [OH-] = 3.9 x 10^-5M is:

• 4.41
• 3.90
• 9.59
• 4.80