How many ml of 1.50 m hcl are needed to titrate 25.0 ml of 1.20 m ca (oh) 2?

The balanced chemical equation for the above reaction is as follows;

Ca (OH) ₂ + 2HCl - - > CaCl₂ + 2H₂O

stoichiometry of Ca (OH) ₂ to HCl is 1:2

The number of Ca (OH) ₂ moles required - 1.2 M / 1000 mL/L x 25.0 mL = 0.03 mol

number of HCl moles required for complete neutralisation - 0.03 x 2 = 0.06 mol

the molarity of HCl solution - 1.50 M

There are 1.50 mol in 1 L solution

Therefore 0.06 mol of HCl in - 1/1.50 x 0.06 = 0.04 L

therefore volume of HCl required is 40 mL