Write balanced net ionic equations for the following reactions in acidic solution. (a)

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Identify the reactants and products involved in the reaction.

Write the balanced molecular equation for the reaction.

Separate the aqueous compounds into their respective ions to write the complete ionic equation.

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

Write the net ionic equation, including only the species that undergo a change.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Net Ionic Equations

Net ionic equations represent the actual chemical species that participate in a reaction, excluding spectator ions. They are derived from complete ionic equations by removing ions that do not change during the reaction. This simplification helps to focus on the essential chemical changes occurring in the solution.

Acidic Solution

An acidic solution is characterized by a higher concentration of hydrogen ions (H⁺) than hydroxide ions (OH⁻). In such solutions, acids donate protons to the reaction, influencing the behavior of reactants and products. Understanding the properties of acids and their dissociation in water is crucial for predicting the outcome of reactions in acidic environments.

Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the equation, adhering to the law of conservation of mass. This process often involves adjusting coefficients to achieve balance, which is essential for accurately representing the stoichiometry of the reaction and predicting the amounts of reactants and products involved.

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