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What is the molarity of sodium ions in 0.1 mol L^-1 sodium sulphate solution, assuming complete ionisation?
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Answer and explanation
Correct answer: 0.20 mol L^-1
Sodium sulphate dissociates ideally as Na2SO4 → 2Na+ + SO4^2−. Thus every 1 mol of Na2SO4 produces 2 mol of Na+. For a 0.1 mol L^-1 solution, sodium-ion concentration is 2 × 0.1 = 0.20 mol L^-1. The coefficient 2 before Na+ is the essential stoichiometric factor.
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What is the correct answer to this question?
0.20 mol L^-1
Why is this the correct answer?
Sodium sulphate dissociates ideally as Na2SO4 → 2Na+ + SO4^2−. Thus every 1 mol of Na2SO4 produces 2 mol of Na+. For a 0.1 mol L^-1 solution, sodium-ion concentration is 2 × 0.1 = 0.20 mol L^-1. The coefficient 2 before Na+ is the essential stoichiometric factor.
Which subject and chapter does this question cover?
This is a Class 11 Chemistry question. Chapter: Chapter 01: Solutions.
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