Steps for solving titration problems Balanced neutralization equation Volume & concentration of base -> mols OH- mols OH- to mols H3O+ mols H3O+ to mols acid mols acid & volume acid to concentration of acid

Practice Titration Problem In a titration, 27.4 mL of 0.0154M barium hydroxide solution is added to a 20.0 mL sample of hydrochloric acid solution of unknown concentration. What is the molarity of the acid solution?

1) Ba(OH)2 + 2 HCl -> BaCl2 + 2H2O 2) 27.4mLBa(OH)2 x 1 L Ba(OH)2 x 0.0154 molBa(OH)2 x 1000mLBa(OH)2 1 L Ba(OH)2 2 mol OH- = 8.4392 x 10-4 mol OH- 1 mol Ba(OH)2 3) 8.4392 x 10-4 mol OH- = 8.4392 x 10-4 mol H3O+ 4) 8.4392 x 10-4 mol H3O+ x 1 mol HCl = 8.4392 x 10-4 mol HCl 1 mol H3O+ 5) M = mol/L, so ... 8.4392 x 10-4 mol HCl / 0.0200L HCl Final Answer: 0.0422 M HCl