Question

What is the molar it's if the HBr solution if 0.500 liters are titrated to an endpoint by 0.100 liters of a 2.00 M KOH solution

Answer 1

0.4 M

Step-by-step explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

HBr + KOH —> KBr + H₂O

From the balanced equation above,

The mole ratio of the acid, HBr (nₐ) = 1

The mole ratio of the base, KOH (n₆) = 1

Finally, we shall determine the molarity of HBr. This can be obtained as follow:

Volume of acid, HBr (Vₐ) = 0.5 L

Volume of base, KOH (V₆) = 0.1 L

Molarity of base, KOH (M₆) = 2 M

Molarity of acid, HBr (Mₐ) =?

MₐVₐ / M₆V₆ = nₐ/n₆

Mₐ × 0.5 / 2 × 0.1 = 1

Mₐ × 0.5 / 0.2 = 1

Cross multiply

Mₐ × 0.5 = 0.2

Divide both side by 0.5

Mₐ = 0.2 / 0.5

Mₐ = 0.4 M

Thus, the molarity of the HBr solution is 0.4 M