Write a balanced net ionic equation for each of the following reactions. (a) Zn(s) + dilute H2SO4(aq) → ? (b) BaSO3(s) + HCl(aq) → ? (c) Cu(s) + hot, concentrated H2SO4(l) → ? (d) H2S(aq) + I2(aq) → ?

Verified step by step guidance

1. Step 1: Identify the reactants and products for each reaction. For example, in reaction (a), the reactants are Zn(s) and H2SO4(aq), and the products are ZnSO4(aq) and H2(g).
2. Step 2: Write the complete ionic equation for each reaction by breaking down all aqueous compounds into their respective ions. For example, in reaction (a), H2SO4(aq) dissociates into 2H+(aq) and SO4^2-(aq).
3. Step 3: Identify and cancel out the spectator ions that appear on both sides of the complete ionic equation. Spectator ions do not participate in the actual chemical change.
4. Step 4: Write the net ionic equation by including only the species that undergo a change. For example, in reaction (a), the net ionic equation would involve Zn(s) and H+(aq) forming Zn^2+(aq) and H2(g).
5. Step 5: Ensure that the net ionic equation is balanced in terms of both mass and charge. Check that the number of atoms and the total charge are the same on both sides of the equation.

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 solution.

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between species, resulting in changes in oxidation states. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Understanding redox processes is crucial for predicting the products of reactions involving metals and acids.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In aqueous solutions, acids donate protons while bases accept them. Recognizing the acid-base nature of reactants is essential for writing balanced equations, especially when dealing with reactions involving strong acids and their salts.