Question

✍️ QUESTION:

Molarity of 20ml of $\sf {H_{2}SO&{4}}$ that can exactly neutralise 5ml of 1M NaOH is ?

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Answer 1

Answer :-

Required Molarity of H₂SO₄ is 0.125 M .

Explanation :-

We have :-

→ Volume of H₂SO₄ (V₁) = 20 mL

→ Volume of NaOH (V₂) = 5 mL

→ Molarity of NaOH (M₂) = 1 M

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H₂SO₄ + 2NaOH → Na₂SO4 + 2H₂O

For this chemical reaction, we have :-

• n-factor of H₂SO₄ = 2

• n-factor of NaOH = 1

Also, we know that :-

⇒ Normality = Molarity × n-factor

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Now for normality based on volumetric analysis, we have the formula :-

N₁V₁ = N₂V₂

⇒ (M₁ × n-factor)V₁ = (M₂ × n-factor)V₂

⇒ (M₁ × 2) × 20 = (1 × 1) × 5

⇒ 2M₁ × 20 = 5

⇒ 40M₁ = 5

⇒ M₁ = 5/40

⇒ M₁ = 0.125 M

Answer 2

Given :-

Molarity of 20ml of H₂SO4 that can exactly neutralize 5ml of 1M

To Find :-

Molarity

Solution :-

Equation formed

2NaOH + H₂SO4 ⇒ 2H₂O + Na₂SO4

Here

NaOH = Base = Sodium hydroxide

H₂SO4 = Acid = Sulfuric acid

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Na = 2                                   Na = 2

O = 5                                      O = 5

S = 1                                        S = 1

H = 4                                       H = 4

Hence, it is balanced

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We know that,

the product of the normality and the volume of the reacting material (acid, bases) are equally distributed.

N1V1 = N2V2

Let the molarity be x

(x)(2)(20) = (1)(1)(5)

2x(20) = 5

40x = 5

x = 5/40

x = 1/8

Hence

Molarity is 1/8 M or 0.125 M