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galben [10]
3 years ago
5

A 49.48-mL sample of an ammonia solution is analyzed by titration with HCl. It took 38.73 mL of 0.0952 M HCl to titrate the ammo

nia. What is the concentration of the original ammonia solution?
Chemistry
1 answer:
Kryger [21]3 years ago
8 0

Answer:

M₂ = 0.0745 M

Explanation:

In case of titration , the following formula can be used -

M₁V₁ = M₂V₂

where ,

M₁ = concentration of acid ,

V₁ = volume of acid ,

M₂ = concentration of base,

V₂ = volume of base .

from , the question ,

M₁ = 0.0952 M

V₁ = 38.73 mL

M₂ = ?

V₂ = 49.48 mL

Using the above formula , the molarity of ammonia , can be calculated as ,

M₁V₁ = M₂V₂  

0.0952 M * 38.73 mL = M₂* 49.48 mL

M₂ = 0.0745 M

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For the formation of ammonia, NH3, the enthalpy of reaction is shown:
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<u>Answer:</u> The amount of energy required to convert ammonia back to hydrogen and nitrogen is 45.9 kJ

<u>Explanation:</u>

Endothermic reactions are defined as the reactions in which energy is absorbed in the reaction. The enthalpy change of the reaction is positive.

Exothermic reactions are defined as the reactions in which energy is released in the reaction. The enthalpy change of the reaction is negative.

For the given chemical equation:

3H_2(g)+N_2(g)\rightarrow 2NH_3(g);\Delta H=-45.9kJ

In the above reaction, the enthalpy change is negative. So, the reaction is exothermic in nature.

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