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Ch.5 - Introduction to Solutions and Aqueous Solutions
All textbooksTro 5th EditionCh.5 - Introduction to Solutions and Aqueous SolutionsProblem 56b,c
Chapter 5, Problem 56b,c

Write balanced complete ionic and net ionic equations for each acid–base reaction.
b. HCHO2(aq) + NaOH(aq) →
c. HC2H3O2(aq) + LiOH(aq) →

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Identify the reactants and products in the given acid-base reaction: HCHO_2 (formic acid) and NaOH (sodium hydroxide).
Write the balanced molecular equation for the reaction: HCHO_2(aq) + NaOH(aq) \rightarrow NaCHO_2(aq) + H_2O(l).
Break down all the strong electrolytes into their ions to write the complete ionic equation: HCHO_2(aq) + Na^+(aq) + OH^-(aq) \rightarrow Na^+(aq) + CHO_2^-(aq) + H_2O(l).
Identify the spectator ions, which are ions that appear on both sides of the complete ionic equation and do not participate in the reaction. In this case, Na^+ is the spectator ion.
Write the net ionic equation by removing the spectator ions: HCHO_2(aq) + OH^-(aq) \rightarrow CHO_2^-(aq) + H_2O(l).

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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 context, HCHO2 (formic acid) acts as an acid, donating a proton, while NaOH (sodium hydroxide) serves as a base, accepting the proton. Understanding the roles of acids and bases is crucial for writing balanced equations.
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Complete Ionic Equations

A complete ionic equation represents all the ions present in a solution during a reaction. It shows the reactants and products in their ionic forms, highlighting the dissociation of soluble ionic compounds. This step is essential for identifying the species involved in the reaction before simplifying to the net ionic equation.
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Net Ionic Equations

A net ionic equation focuses on the species that actually participate in the reaction, omitting spectator ions that do not change during the reaction. By removing these non-reactive ions, the net ionic equation provides a clearer picture of the chemical change occurring, which is particularly useful in acid-base reactions.
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Related Practice
Textbook Question

Complete and balance each acid–base equation.

a. H2SO4(aq) + Ca(OH)2(aq) →

b. HClO4(aq) + KOH(aq) →

c. H2SO4(aq) + NaOH(aq) →

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Textbook Question

Complete and balance each acid–base equation. b. HC2H3O2(aq) + Ca(OH)2(aq) →

Textbook Question

Write balanced complete ionic and net ionic equations for each acid–base reaction. a. HI(aq) + RbOH(aq) →

Textbook Question

A 25.00-mL sample of an unknown HClO4 solution requires titration with 22.62 mL of 0.2000 M NaOH to reach the equivalence point. What is the concentration of the unknown HClO4 solution? The neutralization reaction is HClO4(aq) + NaOH(aq) → H2O(l) + NaClO4(aq)

Textbook Question

A 30.00-mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.38 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is H3PO4(aq) + 3 NaOH(aq) → 3 H2O(l) + Na3PO4(aq)

Textbook Question

Complete and balance each gas-evolution equation. b. NH4I(aq) + NaOH(aq) →

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