Textbook Question
Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. potassium carbonate and lead(II) nitrate
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Ch.5 - Introduction to Solutions and Aqueous Solutions
Chapter 5, Problem 47a
Write balanced complete ionic and net ionic equations for each reaction. a. HCl(aq) + LiOH(aq) → H2O(l) + LiCl(aq)
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Identify the reactants and products in the given chemical equation: HCl(aq) + LiOH(aq) \rightarrow H_2O(l) + LiCl(aq).
Write the balanced molecular equation: HCl(aq) + LiOH(aq) \rightarrow H_2O(l) + LiCl(aq).
Write the complete ionic equation by separating all strong electrolytes into their ions: H^+(aq) + Cl^-(aq) + Li^+(aq) + OH^-(aq) \rightarrow H_2O(l) + Li^+(aq) + Cl^-(aq).
Identify and cancel out the spectator ions, which appear on both sides of the complete ionic equation: Li^+(aq) and Cl^-(aq).
Write the net ionic equation by including only the ions and molecules directly involved in the reaction: H^+(aq) + OH^-(aq) \rightarrow H_2O(l).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Complete Ionic Equation
A complete ionic equation represents all the ions present in a solution during a chemical reaction. It shows the reactants and products in their ionic forms, highlighting the dissociation of soluble ionic compounds in aqueous solutions. This equation is essential for understanding how ions interact in solution and sets the stage for identifying the net ionic equation.
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Complete Ionic Equations
Net Ionic Equation
The net ionic equation simplifies the complete ionic equation by removing spectator ions—ions that do not participate in the actual chemical reaction. This equation focuses solely on the species that undergo a change, providing a clearer picture of the chemical process. It is particularly useful for emphasizing the essential components of a reaction and understanding the underlying chemistry.
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Acid-Base Neutralization Reaction
An acid-base neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In the given reaction, hydrochloric acid (HCl) reacts with lithium hydroxide (LiOH), resulting in the formation of water (H2O) and lithium chloride (LiCl). Understanding this type of reaction is crucial for predicting the products and writing the corresponding ionic equations.
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Related Practice
Textbook Question
Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' c. copper(II) nitrate and magnesium sulfide
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Textbook Question
Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate
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Textbook Question
Write balanced complete ionic and net ionic equations for each reaction. CaS(aq) + CuCl2(aq) → CuS(s) + CaCl2(aq)
Textbook Question
Write balanced complete ionic and net ionic equations for each reaction. d. Na3PO4(aq) + NiCl2(aq) → Ni3(PO4)2(s) + NaCl(aq)
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Textbook Question
Write balanced complete ionic and net ionic equations for each reaction. a. K2SO4(aq) + CaI2(aq) → CaSO4(s) + KI(aq)