a. Calculate the volume of 0.450 M Ba(OH), which will be needed to neutralize 46,00 mL of 0.252 M HCI.

 b. Find the molar concentration of a sulfuric acid solution, 35.00 mL of which neutralizes 25.00 mL of 0.320 M NaOH. (Careful! Sulfuric acid is diprotic!)

 c. Calculate the "molarity of water" H₂O in pure water at 30°C. (Hint: The density of water at 30°C is 0.9957 g/mL.]

 d. A 15.00 mL sample of a solution of H₂SO₄ of unknown concentration was titrated with 0.3200 N NaOH. The titration required 21.30 mL of the base. Assuming complete neutralization of the acid, 

  i) What was the normality of the acid solution?

  ii) What was the molarity of the acid solution?