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: The volume of Barium hydroxide require is 110milliLitres

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