The net ionic equation is:

Answer: H+(aq) + OH-(aq) - H2O(l) Strong acid + strong base: spectator ions Na+ and Cl- cancel, leaving H+ + OH- - H2O.

Answer: Bronsted-Lowry base (proton acceptor) NH3 accepts a proton from water to form NH4+, defining a Bronsted-Lowry base.

Which is a strong acid?

Answer: Hydrochloric acid (HCl) Common strong acids: HCl, HBr, HI, HNO₃, H₂SO₄, HClO₄, HClO₃. They fully dissociate in water.

AP Chemistry · Topic 4.8

Acid-Base Reactions Practice

Part of Chemical Reactions.(TRA-2.B)

Practice questions

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Sample questions

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Sample 1difficulty 1/5
$The net ionic equation is:$
- A
  $Na+ + Cl- -> NaCl$
- B
  $H+ + Cl- -> HCl$
- C
  $H+(aq) + OH-(aq) -> H2O(l)$
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- D
  $HCl + NaOH -> NaCl + H2O$
Why
$Strong acid + strong base: spectator ions Na+ and Cl- cancel, leaving H+ + OH- -> H2O.$
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Sample 2difficulty 1/5
$NH3 acts as the:$
- A
  $Bronsted-Lowry base (proton acceptor)$
  check_circle
- B
  $Catalyst$
- C
  $Bronsted-Lowry acid$
- D
  $Lewis acid$
Why
$NH3 accepts a proton from water to form NH4+, defining a Bronsted-Lowry base.$
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Sample 3difficulty 2/5
$Which is a strong acid?$
- A
  $Carbonic acid (H₂CO₃)$
- B
  $Hydrofluoric acid (HF)$
- C
  $Hydrochloric acid (HCl)$
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- D
  $Acetic acid (CH₃COOH)$
Why
$Common strong acids: HCl, HBr, HI, HNO₃, H₂SO₄, HClO₄, HClO₃. They fully dissociate in water.$
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Sample 4difficulty 2/5
$Which is a strong base?$
- A
  $Mg(OH)₂$
- B
  $NH₃$
- C
  $NaOH$
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- D
  $CH₃NH₂$
Why
$Group 1 hydroxides (NaOH, KOH, LiOH, etc.) and heavier Group 2 hydroxides are strong bases (fully dissociate).$
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Sample 5difficulty 2/5
$The neutralization reaction HCl + NaOH \to NaCl + H₂O has the net ionic equation$
- A
  $All species participate$
- B
  $Na⁺ + Cl⁻ \to NaCl$
- C
  $HCl + NaOH \to NaCl + H₂O$
- D
  $H⁺ + OH⁻ \to H₂O$
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Why
$Strong acid + strong base. Na⁺ and Cl⁻ are spectators.$
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