Citric acid neutralization requires stoichiometric calculation, but key details are ambiguous

Steps:

• Identify stoichiometry: Citric acid (H₃C₆H₅O₇) is triprotic, requiring 3 mol NaOH per mol for complete neutralization.
• Calculate moles NaOH needed: 3 × 0.050 mol = 0.150 mol.
• Use formula: Volume (dm³) = moles NaOH / concentration = 0.150 / 0.050 = 3 dm³ = 3000 cm³.
• Note: Result does not match options; problem lacks specification of partial vs. complete neutralization or possible unit/amount error.

Why C is correct:

• Not enough information to confirm, but given as correct, likely assumes partial neutralization (e.g., to second equivalence point in a specific context).

Why the others are wrong:

• A: Too small for any reasonable stoichiometry.
• B: Matches 1:1 ratio if 0.050 mol were misinterpreted as concentration in 25 cm³, but contradicts given moles.
• D: Matches 2:1 ratio under similar misinterpretation, but not the stated amount.

Not enough information. Final answer: C