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A student cleaned their glassware with tap water (known to contain chloride ions). They then attempted to make a 0.020 M solution of silver nitrate from a stock solution of 0.10 M silver nitrate and immediately noticed a white precipitate. Write the net ionic equation for the formation of the precipitate. Include states of matter.

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Answer:

Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

Explanation:

The silver nitrate, AgNO₃, dissolves in water as follows:

AgNO₃(aq) → Ag⁺(aq) + NO₃⁻(aq)

The Ag⁺ reacts with Cl⁻ producing AgCl(s), a white insoluble salt. The net ionic equation that describes the formation of the precipitate is:

Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

The net ionic equation for the formation of the precipitate. Include states of matter is Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

The following information should be considered:

  • The silver nitrate, AgNO₃, dissolves in water should be  

AgNO₃(aq) → Ag⁺(aq) + NO₃⁻(aq)

  • The Ag⁺ reacts with Cl⁻  generatedAgCl(s), a white insoluble salt.

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