May 07, 2021, 10:17:31 PM
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Topic: Neutralisation  (Read 368 times)

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Offline Sam1988

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Neutralisation
« on: March 04, 2021, 06:33:01 AM »
These may seem like strange questions.

1) What is the real definition of neutralisation if these reactions are considered neutralisation reactions ?

A)Sodium hydroxide and hydrochloric acid (salt and water product, pH7)
B) ammonia and hydrochloric acid in solution  ( Salt formed but is a weak acid, no water and pH below 7)
C)  ammonia and hydrogen chloride gas ( solid Salt formed that would be a a weak acid in solution )


2)
a) secondly, are all acid base reactions neutralisation reaction or are neutralisation reactions a subgroup of acid base reactions?

B) Can you consider Na2O + H2O -> 2NaOH a neutralisation reaction because Na2O is the base and Water is the acid?

Offline billnotgatez

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Re: Neutralisation
« Reply #1 on: March 04, 2021, 07:13:10 AM »
We only post a given question once on the forum.
This is a forum policy.
Click on the link near the top center of the forum page.
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http://www.chemicalforums.com/index.php?topic=65859.0

I deleted the duplicate on the other board

Offline Orcio_Dojek

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Re: Neutralisation
« Reply #2 on: March 10, 2021, 03:26:10 PM »
Quote
1) What is the real definition of neutralisation if these reactions are considered neutralisation reactions ?

A)Sodium hydroxide and hydrochloric acid (salt and water product, pH7)
B) ammonia and hydrochloric acid in solution  ( Salt formed but is a weak acid, no water and pH below 7)
C)  ammonia and hydrogen chloride gas ( solid Salt formed that would be a a weak acid in solution )

A reaction which product gives solution closer to neutral (7 - water) pH than reaction substrats.

Quote
2)
a) secondly, are all acid base reactions neutralisation reaction or are neutralisation reactions a subgroup of acid base reactions?

No, because..

Na2O + H2O -> 2 NaOH

gives solution far away from neutral.

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