In a titration, 25.9 ml of 3.4 x10^-3 m ba(oh)2 neutralized 16.6 ml of hcl solution. what is the molarity of the hcl solution?

First, We have to write the equation for neutralization:
Ba(OH)2 + 2HCl → BaCl2 + 2H2O 
so, from the equation of neutralization, we can get the ratio between Ba(OH)2 and HCl. Ba(OH)2 : HCl = 1:2 
- We have to get the no.of moles of Ba(OH)2 to do the neutralization as we have 25.9ml of 3.4 x 10^-3 M Ba(OH)2.
So no.of moles of Ba(OH)2 = (25.9ml/1000) * 3.4x10^-3 = 8.8 x 10^-5 mol
and when Ba(OH)2 : HCl = 1: 2 
So the no.of moles of HCl = 2 * ( 8.8x10^-5) =  1.76 x 10^-4 mol

So when we have 1.76X10^-4 Mol in 16.6 ml (and we need to get it per liter)
∴ the molarity = no.of moles / mass weight
                        = (1.76 x 10^-4 / 16.6ml)* (1000ml/L) = 0.0106 M Hcl

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