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Ch.5 - Introduction to Solutions and Aqueous Solutions
All textbooksTro 6th EditionCh.5 - Introduction to Solutions and Aqueous SolutionsProblem 87a
Chapter 5, Problem 87a

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' a. HCl(aq) + Hg2(NO3)2(aq) →

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Identify the reactants: Hydrochloric acid (HCl) and Mercury(I) nitrate (Hg_2(NO_3)_2).
Determine the possible products by considering the exchange of ions: Hg_2Cl_2 and HNO_3.
Write the unbalanced molecular equation: HCl(aq) + Hg_2(NO_3)_2(aq) → Hg_2Cl_2(s) + HNO_3(aq).
Balance the chemical equation by ensuring the number of atoms of each element is the same on both sides.
Check the solubility of the products: Hg_2Cl_2 is insoluble, confirming the formation of a precipitate.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this case, hydrochloric acid (HCl) acts as an acid, donating a proton, while the mercury(II) nitrate (Hg2(NO3)2) can act as a base. Understanding the nature of these reactants is crucial for predicting the products of the reaction.
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Balancing Chemical Equations

Balancing chemical equations is essential to ensure that the law of conservation of mass is upheld, meaning the number of atoms of each element must be the same on both sides of the equation. This involves adjusting coefficients in front of compounds to achieve balance, which is a fundamental skill in chemistry.
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Solubility Rules

Solubility rules help predict whether a reaction will occur in aqueous solutions based on the solubility of the products formed. For instance, if a product is insoluble, it may precipitate out of solution, indicating a reaction has taken place. In this case, knowing the solubility of mercury compounds is key to determining the outcome of the reaction.
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Related Practice
Textbook Question

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. Al(s) + 3 Ag+(aq) → Al3+(aq) + 3 Ag(s) b. SO3(g) + H2O(l) → H2SO4(aq) c. Ba(s) + Cl2(g) → BaCl2(s) d. Mg(s) + Br2(l) → MgBr2(s)

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Find the percent by mass of sodium chloride in a 1.12 M NaCl solution. The density of the solution is 1.04 g/mL.

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