A solution containing 12.25 g of a strong monoprotic acid is neutralized by 100 ml of 2.5 M KOH. Identify the acid.
- HCl
- H₂SO₄
- HNO₃
- HClO₄
📝 Detailed explanation
Moles KOH = 0.1 L × 2.5 M = 0.25 mol.Since the acid is monoprotic (HA), moles of acid = 0.25 mol.
Molar mass = 12.25 / 0.25 = 49 g/mol.
Checking masses: HCl(36.5), HNO₃(63), HClO₄(100.5).
If the acid was diprotic like H₂SO₄ (98 g/mol), 0.125 mol would weigh 12.25g.
Given "monoprotic", check HClO₄ or others.
None of the common acids match 49 g/mol.
If the mass was 9.125g, it would be HCl.
If the acid is Phosphoric (H₃PO₄ is triprotic), M=98.
Let's assume HClO₄ and re-check titration values.
If moles KOH = 0.25, and acid is 12.25g, M = 49.
This likely refers to H₂SO₄ acting as monoprotic in first stage, but usually M=49 refers to equivalent mass.