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alexira [117]
3 years ago
7

Which one of the following equations represents the net ionic equation for the reaction between aqueous potassium chloride and a

queous silver nitrate? A. Cl- (aq) + Ag+ (aq) AgCl (s) B. K+ (aq) + Cl- (aq) + Ag+ (aq) + NO3- (aq) AgCl (s) + K+ (aq) + NO3- (aq) C. KCl (aq) + AgNO3 (aq) AgCl (s) + KNO3 (aq) D. K+ (aq) + NO3- (aq) KNO3 (aq)
Chemistry
1 answer:
Nana76 [90]3 years ago
4 0
<h3>Answer:</h3>

Ag⁺(aq) +Cl⁻(aq) → AgCl(s)

<h3>Explanation:</h3>

The questions requires we write the net ionic equation for the reaction between aqueous potassium chloride and aqueous silver nitrate.

<h3>Step 1: Writing a balanced equation for the reaction.</h3>
  • The balanced equation for the reaction between aqueous potassium chloride and aqueous silver nitrate will be given by;

KCl(aq) + AgNO₃(aq) → KNO₃(aq) +AgCl(s)

  • AgCl is the precipitate formed by the reaction.
<h3>Step 2: Write the complete ionic equation.</h3>
  • The complete ionic equation for the reaction is given by showing all the ions involved in the reaction.

K⁺(aq)Cl⁻(aq) + Ag⁺(aq)NO₃⁻(aq) → K⁺(aq)NO₃⁻(aq) +AgCl(s)

  • Only ionic compounds are split into ions.
<h3>Step 3: Write the net ionic equation for the reaction.</h3>
  • The net ionic equation for a reactions only the ions that fully participated in the reaction and omits the ions that did not participate in the reaction.
  • The ions that are not involved directly in the reaction are known as spectator ions and are not included while writing net ionic equation.

Ag⁺(aq) +Cl⁻(aq) → AgCl(s)

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From my understanding of the question, we are required to identify the

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