Question

27.64 ml of 0.500 M HCl is required to titrate 10.0 ml of barium hydroxide solution. what is the concentration of the barium hydroxide solution?

Answer 1

In order to ascertain the concentration of barium hydroxide with the given data, we would first write the balanced chemical equation for the reaction:

2HCl + Ba(OH)2 + 2H2O + BaCl2

From the equation, we can see that 2 mole of HCl reacts with 1 mole of Ba(OH)2

Now, we'll first calculate the moles of HCl reacted in the reaction:

moles of HCl = Molarity x Volume of HCI

mol moles of HCl = 0.500– IL -X 27.64 1000

moles of HCl = 0.0138 mol

Now, from this, we can ascertain the number of moles of barium hydroxide required to react with 0.0138 mol of HCl.

1 mol of Ba(OH)2 0.0138 mol HCI X – = = 0.0069 mol of Ba(OH)2 2 mol of HCI

From this, we can ascertain the molarity of barium hydroxide.

0.0069 moles Concentration of Ba(OH)2 = - 0.010 L

Concentration of Ba(OH)2 = 0.69 M