Question

I need help, the longer I look at this question the more I confuse myself!!!
Consider the unbalanced equation:
HC2H3O2 (aq) +Ba(OH)2 (aq) --> H2O (l) +Ba(C2H3O2)2 (aq)

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

Answer 1

First start by balancing the equation. You only have one of the C2H3O2 groups on the reactant side and 2 on the product side, so 2HC2H3O2 + Ba(OH)2 -> H2O + Ba(C2H3O2)2 is the first step. Since we have balanced Ba's, I'll look at the hydrogens next. If we have 2 mols of H2O, the hydrogens will be balanced, so 2HC2H3O2 + Ba(OH)2 -> 2H2O + Ba(C2H3O2)2. Check all individual elements and this checks out! So now, we know that for every 2 mols of HC2H3O2 we will need 1 mol of Ba(OH)2 to neutralize (make the reaction go to completion). 0.461 mol HC2H3O2 (1 mol Ba(OH)2/2mol HC2H3O2) = 0.231 mol Ba(OH)2. Make sense?

Answer 2

The computer will not accept this balanced equation. It says there is something wrong with the format.

Answer 3

Hmm not sure what is wrong with the format (or the computer program). Does it make sense to you logically when you work it out on paper?