5 litres of 2 M H₂SO₄ and 2 litres of 1 M NaOH are mixed with each other.The solution is diluted to ten litres.  Proton concentration of the resultant mixture is ----- M

Complete Solution:

Moles of H₂SO₄:

Moles = 5 L × 2 M = 10 mol

Since H₂SO₄ is a diprotic acid, it releases 2 moles of H⁺ per mole:

Moles of H⁺ from H₂SO₄ = 10 × 2 = 20 mol

Moles of NaOH:

Moles = 2 L × 1 M = 2 mol

NaOH provides 1 mole of OH⁻ per mole.

Determine the Reaction Between H₂SO₄ and NaOH:

Reaction: 2H⁺ + OH⁻ → H₂O

Moles of H⁺ Reacted: 2 mol (since NaOH provides 2 mol of OH⁻)

Remaining Moles of H⁺: 20 mol (initial H⁺) - 2 mol (reacted) = 18 mol

Calculate Proton Concentration After Dilution:

Final Volume: 10 L

Concentration of H⁺: [H⁺] = 18 mol / 10 L = 1.8 M

Final Answer:

The proton concentration of the resultant mixture is 1.8 M.