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?

Expert Answers

An illustration of the letter 'A' in a speech bubbles

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...

Unlock
This Answer Now

Start your 48-hour free trial to unlock this answer and thousands more. Enjoy eNotes ad-free and cancel anytime.

Start your 48-Hour Free Trial

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`

Approved by eNotes Editorial Team