Question

How many milliliters of a 0.70 M solution of barium hydroxide, Ba(OH)2 , are necessary to neutralize 55 mL of a 1.4 M solution of sulfuric acid, H2SO4?

Answer 1

Answer: The volume of Barium hydroxide require is 110milliLitres

Step-by-step explanation:

The neutralization equation;

Ba(OH)2 (aq) + H2SO4 (aq) → BaSO4 (s) + 2H20(1)

Using the relation

CaVa/CbVb = Na/Nb

Ca= molar concentration of acid=1.4M

Cb=molar concentration of base=?

Va= volume of acid =55mL

Vb= Volume of base =?

Na= mole of acid from stoichiometric equations =1

Nb= mole of base from stoichiometric equation 1

(1.4 × 55)/(0.7 ×Vb) = 1/1

Vb= 110mL

Therefore the volume of Ba(OH)2 requires to neutralize the Sulfuric acid is 110millilitres