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

Verified step by step guidance

1. insert step 1: Identify the reactants and products in the given chemical reaction.
2. insert step 2: Write the balanced molecular equation for the reaction.
3. insert step 3: Separate the aqueous compounds into their respective ions to write the complete ionic equation.
4. insert step 4: Identify and cancel out the spectator ions to derive the net ionic equation.
5. insert step 5: Ensure the net ionic equation is balanced in terms of both mass and charge, and adjust for basic conditions by adding OH⁻ ions if necessary.

Key Concepts

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 components and the changes occurring in the reaction.

Basic Solution

A basic solution has a pH greater than 7 and contains hydroxide ions (OH-). In such solutions, reactions may involve the addition of hydroxide ions to neutralize acids or to facilitate the formation of precipitates. Understanding the behavior of species in basic conditions is crucial for accurately writing net ionic equations.

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 and may require accounting for charges in ionic reactions, especially in net ionic equations where charge balance is critical.