Both salts acidify neutral soil equally due to ammonium hydrolysis Steps:

• Calculate %N in NH4NO3: molar mass 80 g/mol, N mass 14 g/mol, so %N = (14/80) × 100 = 17.5%.
• Calculate %N in (NH4)2SO4: molar mass 132 g/mol, N mass 28 g/mol, so %N = (28/132) × 100 ≈ 21.2%.
• Both contain NH4+ ions, which hydrolyze in water: NH4+ + H2O ⇌ NH3 + H3O+, producing H+ and decreasing pH.
• Anions SO4^2- and NO3- are from strong acids, so neither buffers the acidity; both salts decrease pH equally.

Why A is correct:

• Option A correctly identifies NH4NO3 with lower %N (17.5%) and pH decrease, matching hydrolysis effect.

Why the others are wrong:

• B incorrectly assigns pH decrease only to (NH4)2SO4, ignoring equal effect on both.
• C repeats B's error with same misattribution.
• D wrongly states (NH4)2SO4 increases pH, contradicting acidic hydrolysis.

Final answer: A