Write a balanced net ionic equation for each of the following reactions. (a) ZnS(s) + HCl(aq) → ? (b) H2S(aq) + Fe(NO3)3(aq) → ? (c) Fe(s) + dilute H2SO4(aq) → ? (d) BaO(s) + H2SO4(aq) → ?

Verified step by step guidance

1. Step 1: Identify the type of reaction for each given equation. For example, ZnS(s) + HCl(aq) is a reaction between a solid and an acid, which may result in the formation of a gas or a soluble product.
2. Step 2: Write the complete ionic equation for each reaction. This involves breaking down all aqueous compounds into their respective ions. For example, HCl(aq) dissociates into H⁺(aq) and Cl⁻(aq).
3. Step 3: Identify and remove the spectator ions from the complete ionic equation. Spectator ions are ions that do not participate in the actual chemical change and appear unchanged on both sides of the equation.
4. Step 4: Write the net ionic equation by including only the ions and molecules directly involved in the chemical reaction. Ensure that the equation is balanced in terms of both mass and charge.
5. Step 5: Verify the physical states of the reactants and products (solid, liquid, gas, aqueous) and ensure that the net ionic equation reflects these states accurately.

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 chemical changes occurring in the reaction.

Solubility Rules

Solubility rules are guidelines that predict whether a compound will dissolve in water. They help determine which reactants will dissociate into ions in solution and which will remain as solids. Understanding these rules is crucial for writing accurate net ionic equations, as they dictate the state of each reactant and product.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In aqueous solutions, acids release H+ ions, while bases accept them. Recognizing the acid-base nature of the reactants is essential for predicting the products and writing balanced equations, particularly in reactions involving strong acids and bases.