Balance the following equations, and then write the net...

Balance the following equations, and then write the net ionic equation. Show states for all reactants and products $(s, \ell, g, a q)$ (a) the reaction of silver nitrate and potassium iodide to give silver iodide and potassium nitrate (b) the reaction of barium hydroxide and nitric acid to give barium nitrate and water (c) the reaction of sodium phosphate and nickel(II) nitrate to give nickel(II) phosphate and sodium nitrate

Balance the following equations, and then write the net ionic equation. Show states for all reactants and products
$(s, \ell, g, a q)$
(a) the reaction of silver nitrate and potassium iodide to give silver iodide and potassium nitrate
(b) the reaction of barium hydroxide and nitric acid to give barium nitrate and water
(c) the reaction of sodium phosphate and nickel(II) nitrate
to give nickel(II) phosphate and sodium nitrate

Key Concepts

Spectator Ions

Spectator ions are ions that do not participate in the actual chemical reaction but remain in the solution unchanged. They appear in identical form on both the reactant and product sides of a complete ionic equation. Removing them helps simplify the equation to highlight the chemistry that is occurring.

Physical States in Chemical Reactions

Indicating the physical states of reactants and products—such as solid (s), liquid (?), gas (g), and aqueous solution (aq)—provides crucial information about the nature of substances in a reaction. This notation helps predict the behavior of the substances, such as solubility and whether a precipitate forms, and is essential for understanding and balancing reactions accurately.

Balancing Chemical Equations

Balancing a chemical equation involves ensuring that the number of atoms for each element is the same on both sides of the reaction. This maintains the law of conservation of mass. In addition, the coefficients used in a balanced equation provide the stoichiometric relationships among the reactants and products, indicating the exact proportions for the reaction to occur without any excess of one substance.

Net Ionic Equations

A net ionic equation represents only the species that undergo a chemical change during the reaction. It is derived by first writing the complete ionic equation, which shows all strong electrolytes dissociated into ions, and then eliminating the ions that appear unchanged on both sides, known as spectator ions. This streamlined form focuses on the actual chemical transformation.

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