AgNO_3(aq) + KCl(aq) \rightarrow AgCl(s) + KNO_3(aq)
Which of the following describes this reaction?
A. precipitation
B. acid-base neutralization
C. redox reaction
Answer (2)
The reaction A g N O 3 ( a q ) + K Cl ( a q ) → A g Cl ( s ) + K N O 3 ( a q ) is analyzed.
It is identified as a precipitation reaction due to the formation of A g Cl ( s ) .
It is not an acid-base neutralization reaction because there are no clear acid or base reactants.
It is not a redox reaction because the oxidation states of the elements do not change.
Therefore, the reaction is a precipitation reaction. p rec i p i t a t i o n
Explanation
Analyzing the Reaction Let's analyze the given chemical reaction to determine its classification.
Identifying the Reaction Type The reaction is: A g N O 3 ( a q ) + K Cl ( a q ) → A g Cl ( s ) + K N O 3 ( a q )
Precipitation: A precipitation reaction involves the formation of an insoluble solid (precipitate) from the reaction of two aqueous solutions. In this reaction, A g Cl is formed as a solid precipitate. Therefore, it is a precipitation reaction.
Acid-Base Neutralization: An acid-base neutralization reaction involves the reaction of an acid and a base to form a salt and water. In this reaction, there are no clear acid or base reactants. Therefore, it is not an acid-base neutralization reaction.
Redox Reaction: A redox reaction involves the transfer of electrons between reactants, resulting in a change in oxidation states. In this reaction, the oxidation states of the elements do not change. For example, the oxidation state of Ag remains +1, K remains +1, N remains +5, O remains -2, and Cl remains -1. Therefore, it is not a redox reaction.
Examples
Precipitation reactions are commonly used in water treatment to remove heavy metals or other contaminants by forming insoluble precipitates that can be filtered out. For example, adding lime (calcium hydroxide) to water can precipitate out magnesium and calcium ions, softening the water. This principle is also applied in various industrial processes to recover valuable metals or remove unwanted impurities from solutions.
The reaction between Silver Nitrate and Potassium Chloride produces Silver Chloride as a solid precipitate, identifying it as a precipitation reaction. It is not an acid-base neutralization or a redox reaction, as there are no acids or bases present and oxidation states do not change. The chosen option is precipitation.
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