Write balanced net ionic equations for the following reactions in basic solution. (c)

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Identify the reactants and products in the given chemical 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 to derive the net ionic equation.

Ensure the net ionic equation is balanced for both mass and charge, and adjust for basic conditions by adding OH⁻ ions if necessary.

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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.

Basic Solution

A basic solution has a pH greater than 7 and contains hydroxide ions (OH-). In such solutions, certain reactions may involve the addition of hydroxide ions to neutralize acids or to form precipitates. Understanding how to manipulate the presence of OH- is crucial for balancing reactions in basic conditions.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is essential for obeying the law of conservation of mass. In the context of net ionic equations, balancing also includes accounting for charge, ensuring that the total charge is equal on both sides.

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