Write a net ionic equation for the reaction that occurs when 10 mL of 0.5 M ammonium carbonate is mixed with 10 mL of 0.5 M silver nitrate. (LO 4.9, 4.11) (a) (b) (c) (d) A net ionic reaction cannot be written because a reaction does not take place.

검증된 단계별 안내

Step 1: Write the balanced molecular equation for the reaction.

Step 2: Identify the states of the reactants and products (solid, liquid, gas, aqueous).

Step 3: Write the complete ionic equation by dissociating all strong electrolytes into their ions.

Step 4: Identify and cancel out the spectator ions that appear on both sides of the complete ionic equation.

Step 5: Write the net ionic equation with the remaining species that participate in the reaction.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Net Ionic Equations

A net ionic equation represents the chemical species that are involved in a reaction, excluding spectator ions that do not participate in the actual chemical change. It focuses on the ions and molecules that undergo a transformation, providing a clearer picture of the reaction's essence. To write a net ionic equation, one must first identify the reactants, their states, and the products formed.

Solubility Rules

Solubility rules are guidelines that help predict whether a compound will dissolve in water. They indicate which ionic compounds are soluble or insoluble in aqueous solutions. Understanding these rules is crucial for determining if a reaction will occur when two solutions are mixed, as insoluble products may precipitate out of solution, leading to a net ionic equation.

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble salt, which precipitates out of the solution. This type of reaction is common in double displacement reactions, where the cations and anions exchange partners. Recognizing whether a precipitate forms is essential for writing the net ionic equation and understanding the overall reaction process.