How much HCl(aq) is necessary to completely neutralize 2 mol of Ba(OH)2(s)?

To determine how much hydrochloric acid (HCl) is necessary to completely neutralize 2 moles of barium hydroxide (Ba(OH)2), it's important to understand the neutralization reaction between an acid and a base. The reaction can be represented as follows:

Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O

In this balanced equation, one mole of barium hydroxide reacts with two moles of hydrochloric acid. Therefore, for every mole of Ba(OH)2, two moles of HCl are required for complete neutralization.

Given that there are 2 moles of Ba(OH)2, the total amount of HCl needed can be calculated by multiplying the number of moles of Ba(OH)2 by the stoichiometric coefficient of HCl from the balanced equation:

2 moles of Ba(OH)2 x 2 moles of HCl per mole of Ba(OH)2 = 4 moles of HCl.

This indicates that to completely neutralize 2 moles of barium hydroxide, 4 moles of hydrochloric acid are indeed necessary. Thus, the answer indicating that 4 moles of