Steps for solving titration problems. Balanced neutralization equation Volume & concentration of base -> mols OH - mols OH - to mols H 3 O + mols H 3 O + to mols acid mols acid & volume acid to concentration of acid. Practice Titration Problem.
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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?
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
1) Ba(OH)2 + 2 HCl -> BaCl2 + 2H2O
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