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A 20.00 mL sample of a Ba(OH)2 solution is titrated with 0.245 M HCl. If 27.15 mL of...

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lak-86 | Student, Undergraduate | Salutatorian

Posted June 11, 2013 at 4:24 AM via web

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A 20.00 mL sample of a Ba(OH)2 solution is titrated with 0.245 M HCl. If 27.15 mL of HCl is required, what is the molarity of the Ba(OH)2 solution?

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jeew-m | College Teacher | (Level 1) Educator Emeritus

Posted June 11, 2013 at 4:37 AM (Answer #1)

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Here we have the equation for the reaction.

`Ba(OH)_2+2HCl rarr BaCl_2+2H_2O`

 

mole ratio

`Ba(OH)_2:HCl = 1:2`

 

Amount of HCl consumed `= 0.245/1000xx27.15 = 0.00665 mol`

 

So amount of `Ba(OH)_2` reacted `= 1/2xx0.00665 mol`

 

Molarity means the amount of moles solute in one litre of solution.

If the molarity of `Ba(OH)_2` is x then;

`x/1000xx20 = 1/2xx0.00665`

`x = 0.1663`

 

So the molarity of the `Ba(OH)_2` solution is `0.1663(mol)/L`

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