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Question

If 200 mL of a standard 0.15 M NaOH solution is required to neutralize 30 ml of H2SO4, what is the molarity of acid? 
 
  1. 2.0 M
  2. 0.5 M
  3. 1.5 M
  4. 1.0 M


Solution

The correct option is B 0.5 M
We have, 
200 mL of a 0.15 M NaOH solution and 30 mL of H2SO4solution of unknown molarity.

Let’s assume the molarity of H2SO4 solution to be M. 
For complete neutralization, 
Number of millimole of H+  ions = Number of millimole of OH  ions
Since, 1 mol of H2SO4 produces 2 mol of H+  ions. i.e. H2SO4  is a diprotic acid
 1×200×0.15=2×30×M
M = 0.5
Therefore the molarity of the acid solution is 0.5 M
 

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