Molarity of silver ion in the original solution if 25.0 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.842 g of precipitate is to be calculated. Concept introduction: Precipitation reaction involves the reaction of two soluble ionic compounds to form an insoluble product. The insoluble product is known as a precipitate. The reason for the precipitation reaction to occur is the formation of a product that is insoluble in nature. The reaction of silver nitrate solution and potassium chloride is an example of precipitation reaction. AgNO 3 ( a q ) + KCl ( a q ) → AgCl ( s ) + KNO 3 ( a q ) According to the solubility rules, all the common nitrates are soluble but AgCl is insoluble in nature.

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Chapter 4, Problem 4.48P

Interpretation Introduction

Interpretation:

Molarity of silver ion in the original solution if 25.0 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.842 g of precipitate is to be calculated.

Concept introduction:

Precipitation reaction involves the reaction of two soluble ionic compounds to form an insoluble product. The insoluble product is known as a precipitate.

The reason for the precipitation reaction to occur is the formation of a product that is insoluble in nature. The reaction of silver nitrate solution and potassium chloride is an example of precipitation reaction.

AgNO3(aq)+KCl(aq)→AgCl(s)+KNO3(aq)

According to the solubility rules, all the common nitrates are soluble but AgCl is insoluble in nature.

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