Question

HC2H3O2(aq) + Ba(OH)2(aq) + ----> H2O(l) + Ba(C2H3O2)(aq)

Balance this equation and determine how many moles of Ba(OH)2 are required to completely neutralize 0.461 mole of HC2H3O2.

Answer 1

The balanced chemical reaction is:

 2HC2H3O2(aq) + Ba(OH)2(aq) + ----> 2H2O(l) + Ba(C2H3O2)2(aq)

We are given the amount of HC2H3O2 to be used in the reaction. This will be the starting point for the calculation.

 0.461 mol HC2H3O2 ( 1 mol Ba(OH)2 / 2 mol HC2H3O2 ) = 0.231 mol Ba(OH)2

Answer 2

Answer: 0.461 moles of $HC_2H_3O_2$

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

$2CH_3COOH(aq)+Ba(OH)_2(aq)\rightarrow 2H_2O(l)+Ba(CH_3COO)_2(aq)$

According to stoichiometry;

2 moles of $HC_2H_3O_2$ require = 1 mole of $Ba(OH)_2$

Thus 0.461 moles of $HC_2H_3O_2$ require = $\frac{1}{2}\times 0.461=0.230$ moles of $Ba(OH)_2$

Thus 0.230 moles $Ba(OH)_2$ are required to completely neutralize 0.461 moles of $HC_2H_3O_2$