Complete and balance each equation. If no reaction occurs, write “NO REACTION.” b. NaCl(aq) + Hg2(C2H3O2)2(aq) → c. (NH4)2SO4(aq) + SrCl2(aq) →

Verified step by step guidance

1. Identify the reactants and products in the given chemical equations.
2. For equation b, NaCl(aq) + Hg2(C2H3O2)2(aq) →, determine if a double displacement reaction occurs by checking the solubility of the potential products: NaC2H3O2 and Hg2Cl2.
3. Use solubility rules to check if any of the products in equation b are insoluble. If one is insoluble, it will precipitate, indicating a reaction occurs.
4. For equation c, (NH4)2SO4(aq) + SrCl2(aq) →, predict the products by swapping the cations and anions to form NH4Cl and SrSO4.
5. Check the solubility of the products in equation c using solubility rules. If SrSO4 is insoluble, it will precipitate, indicating a reaction occurs.

Key Concepts

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 based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas, rather than changing the formulas themselves.

Types of Reactions

Understanding the types of chemical reactions—such as double displacement, single displacement, synthesis, and decomposition—is crucial for predicting the products of a reaction. In double displacement reactions, two compounds exchange ions, which can lead to the formation of a precipitate, gas, or water. Recognizing the type of reaction helps in determining whether a reaction will occur and what the products will be.

Solubility Rules

Solubility rules are guidelines that help predict whether a compound will dissolve in water or form a precipitate. For example, most salts of alkali metals and ammonium are soluble, while many transition metal compounds are not. These rules are essential for determining the outcome of reactions in aqueous solutions, particularly in double displacement reactions where insoluble products may form.