Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Sam1988 on March 04, 2021, 06:33:01 AM
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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?
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http://www.chemicalforums.com/index.php?topic=65859.0 (http://www.chemicalforums.com/index.php?topic=65859.0)
I deleted the duplicate on the other board
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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.
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.