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What volume of 0.062 M HCl is needed to react to completely neutralize 19.4 mL of 0.050 M Ba(OH)2? *

Sagot :

Eduard22sly

Answer:

31.3 mL

Explanation:

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

2HCl + Ba(OH)₂ —> BaCl₂ + 2H₂O

From the balanced equation above,

The mole ratio of the acid, HCl (nₐ) = 2

The mole ratio of the base, Ba(OH)₂ (n₆) = 1

Finally, we shall determine the volume of the acid need for the reaction as follow:

Molarity of acid, HCl (Mₐ) = 0.062 M

Mole ratio of the acid, HCl (nₐ) = 2

Volume of base, Ba(OH)₂ (V₆) = 19.4 mL

Molarity of base, Ba(OH)₂ (M₆) = 0.050 M

Mole ratio of the base, Ba(OH)₂ (n₆) = 1

Volume of acid, HCl (Vₐ) =?

MₐVₐ / M₆V₆ = nₐ / n₆

0.062 × Vₐ / 0.050 × 19.4 = 2/1

0.062 × Vₐ / 0.97 = 2

Cross multiply

0.062 × Vₐ = 0.97 × 2

0.062 × Vₐ = 1.94

Divide both side by 0.062

Vₐ = 1.94 / 0.062

Vₐ = 31.3 mL

Thus, the volume of the acid needed is 31.3 mL

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