Question

1b) If 38.5 mL of 0.225 M HCl solution is needed to neutralize a solution of Ba(OH)2, now many grams of Ba(OH)2 must be in the solution? First write the balanced chemical equation and include state notations.

Answer 1

Balanced equation: 2HCl(aq) + Ba(OH),(aq) → BaCl2 (aq) + H2O(1) Concentration of HC1=0.225 Volume of the HCl solution =38.5mL X- w 1000 mL =0.0385L Number of moles of HC=0.0385L x 0.225 mol = 8.66 x 10-mol molBa(OH), Number of moles of Ba(OH), is needed = 8.66 x 10-molHCIX- 2 mol HCl = 4.33 x 10-molBa(OH), Molar mass of Ba(OH), is 171.33 mole Mass of the Ba(OH), is needed =4.33 x 10 mole x 171. 3 5 mole = 0.7429